This document consists of 18 printed pages and 2 blank pages.
IB13 11_0620_11/2RP © UCLES 2013 [Turn over
*6047676049*
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education
CHEMISTRY 0620/11
Paper 1 Multiple Choice October/November 2013
45 Minutes Additional Materials: Multiple Choice Answer Sheet Soft clean eraser Soft pencil (type B or HB is recommended)
READ THESE INSTRUCTIONS FIRST
Write in soft pencil.
Do not use staples, paper clips, highlighters, glue or correction fluid.
Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless this has been done for you.
DO NOT WRITE IN ANY BARCODES.
There are forty questions on this paper. Answer all questions. For each question there are four possible answers A, B, C and D.
Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.
Read the instructions on the Answer Sheet very carefully.
Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
Any rough working should be done in this booklet.
A copy of the Periodic Table is printed on page 20.
Electronic calculators may be used.
2
© UCLES 2013 0620/11/O/N/13
1 An attempt was made to compress a gas and a solid using the apparatus shown.
piston
gas solid
Which substance would be compressed and what is the reason for this?
substance reason
A gas the gas particles are close together
B gas the gas particles are far apart
C solid the solid particles are close together
D solid the solid particles are far apart
2 A student measures the rate of two reactions.
In one reaction, there is a change in mass of the reactants during the reaction.
In the second reaction, there is a change in temperature during the reaction.
Which piece of apparatus would be essential in both experiments?
A balance
B clock
C pipette
D thermometer
3
© UCLES 2013 0620/11/O/N/13 [Turn over
3 Diagram 1 shows the paper chromatogram of substance X.
R
Y
X
diagram 1
Diagram 2 shows the cooling curve for substance Y.
0
147
0
temperature / °C
time
diagram 2
Which statement about X and Y is correct?
A X is a mixture and Y is a pure substance.
B X is a pure substance and Y is a mixture.
C X and Y are mixtures.
D X and Y are pure substances.
4
© UCLES 2013 0620/11/O/N/13
4 Element X has 7 protons.
Element Y has 8 more protons than X.
Which statement about element Y is correct?
A Y has more electron shells than X.
B Y has more electrons in its outer shell than X.
C Y is in a different group of the Periodic Table from X.
D Y is in the same period of the Periodic Table as X
5 Which statements about a sodium atom, Na,23
11 are correct?
1 The number of protons and neutrons is the same.
2 The number of protons and electrons is the same.
3 The number of outer electrons is one.
A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only 6 Rubidium is in Group I of the Periodic Table and bromine is in Group VII.
Rubidium reacts with bromine to form an ionic compound.
Which row shows the electron change taking place for rubidium and the correct formula of the rubidium ion?
electron change formula of ion formed
A electron gained Rb+
B electron gained Rb–
C electron lost Rb+
D electron lost Rb–
7 The diagrams show the electron arrangements in the atoms of four elements.
Which element does not form a covalent bond?
e e
e e e
e e
e e
e e e e
e e e e
e e key
electron
nucleus
A B C D
e e
e e e e
e e
5
© UCLES 2013 0620/11/O/N/13 [Turn over
8 A solid mixture contains an ionic salt, X, and a covalent organic compound, Y.
Two students suggest methods of separating the mixture as shown.
method 1
method 2
shake withwater
X + Y
shake withethanol
X + Y
Which methods of separation are likely to work?
1 2
A � �
B � �
C � �
D � �
9 The formulae of compounds W, X and Y are shown.
W CuSO4.5H2O
X MgSO4.7H2O
Y Cu(NO3)2.6H2O
Which statement is correct?
A W contains twice as many hydrogen atoms as oxygen atoms.
B X contains the most oxygen atoms.
C Y contains the most hydrogen atoms.
D Y contains the same number of hydrogen and oxygen atoms.
6
© UCLES 2013 0620/11/O/N/13
10 Which relative molecular mass, Mr, is not correct for the molecule given?
molecule Mr
A ammonia, NH3 17
B carbon dioxide, CO2 44
C methane, CH4 16
D oxygen, O2 16
11 The diagram shows the circuit for electrolysing lead(II) bromide and sodium chloride to liberate
the metal.
A
container forlead(II) bromide
container forsodium chloride
In what form are these salts electrolysed for liberating the metal?
lead(II) bromide sodium chloride
A concentrated solution concentrated solution
B concentrated solution molten
C molten concentrated solution
D molten molten
7
© UCLES 2013 0620/11/O/N/13 [Turn over
12 The diagram shows the electrolysis of concentrated aqueous sodium chloride.
+ –anode cathode
concentratedaqueous sodiumchloride and litmus
carbonrods
What is the colour of the litmus at each electrode after five minutes?
colour at anode colour at cathode
A blue red
B red blue
C red colourless
D colourless blue
13 When anhydrous copper(II) sulfate is added to water a solution is formed and heat is given out.
water
anhydrouscopper(II) sulfate
thermometer
Which row correctly shows the temperature change and the type of reaction taking place?
temperature change type of reaction
A decreases endothermic
B decreases exothermic
C increases endothermic
D increases exothermic
8
© UCLES 2013 0620/11/O/N/13
14 Which fuel does not produce carbon dioxide when it burns?
A coal
B hydrogen
C methane
D petrol 15 A student investigates the rate of reaction between zinc and an excess of sulfuric acid.
The graph shows the results of two experiments, X and Y.
0
X
Y
time0
volume ofhydrogen
Which change explains the difference between X and Y?
A A catalyst is added in Y.
B A lower temperature is used in Y.
C Larger pieces of zinc are used in Y.
D Less concentrated acid is used in Y.
16 Anhydrous copper(II) sulfate can be made by heating hydrated copper(II) sulfate.
CuSO4.5H2O → CuSO4 + 5H2O
What can be added to anhydrous copper(II) sulfate to turn it into hydrated copper(II) sulfate?
A concentrated sulfuric acid
B sodium hydroxide powder
C sulfur dioxide
D water
9
© UCLES 2013 0620/11/O/N/13 [Turn over
17 The reactions shown may occur in the air during a thunder storm.
N2 + O2 → 2NO
2NO + O2 → 2NO2
NO + O3 → NO2 + O2
Which row shows what happens to the reactant molecules in each of these reactions?
N2 NO O3
A oxidised oxidised oxidised
B oxidised oxidised reduced
C reduced reduced oxidised
D reduced reduced reduced
18 Which are properties of an acid?
1 reacts with ammonium sulfate to form ammonia
2 turns red litmus blue
1 2
A � �
B � �
C � �
D � �
19 Which of the following are properties of the oxides of non-metals?
property 1 property 2
A acidic covalent
B acidic ionic
C basic covalent
D basic ionic
10
© UCLES 2013 0620/11/O/N/13
20 Compound X is tested and the results are shown in the table.
test result
aqueous sodium hydroxide is
added, then heated gently
gas given off which turns damp
red litmus paper blue
dilute hydrochloric acid is added effervescence, gas given off
which turns limewater milky
Which ions are present in compound X?
A ammonium ions and carbonate ions
B ammonium ions and chloride ions
C calcium ions and carbonate ions
D calcium ions and chloride ions 21 Calcium, on the left of Period 4 of the Periodic Table, is more metallic than bromine on the right of
this period.
Why is this?
Calcium has
A fewer electrons.
B fewer protons.
C fewer full shells of electrons.
D fewer outer shell electrons. 22 The diagrams show the labels of four bottles.
Which label is not correct?
A B C D
Bromine Br2
Harmful liquid.
Do not spill.
Iodine
I2
Danger Avoid breathing vapour
from the solid.
Potassium
K
Danger Store under water.
Sodium
Na
Danger Store under oil.
11
© UCLES 2013 0620/11/O/N/13 [Turn over
23 An element has a melting point of 1084 °C and a density of 8.93 g / cm3. It’s oxide can be used as a catalyst.
In which position in the Periodic Table is the element found?
A B C
D
24 The diagram shows a light bulb.
filament
argon
Why is argon used instead of air in the light bulb?
A Argon is a good conductor of electricity.
B Argon is more reactive than air.
C The filament glows more brightly.
D The filament does not react with the argon. 25 Some properties of four elements W, X, Y and Z are listed.
1 W melts at 1410 °C and forms an acidic oxide.
2 X has a high density and is easily drawn into wires.
3 Y acts as a catalyst and its oxide reacts with acids.
4 Z is a red-brown solid used to make alloys.
Which of the elements are metals?
A 1 and 3 B 2, 3 and 4 C 2 and 3 only D 2 and 4 only
12
© UCLES 2013 0620/11/O/N/13
26 M is a shiny silver metal. It has a melting point of 1455 °C. Many of its compounds are green.
What is metal M?
A aluminium
B copper
C mercury
D nickel 27 Reactions of three metals and their oxides are listed in the table.
metal reacts with cold water
metal oxide reacts with carbon
W no no
X no yes
Y yes no
What is the order of reactivity of the metals?
least reactive most reactive
A W X Y
B X W Y
C X Y W
D Y W X
28 Equations P and Q represent two reactions which occur inside a blast furnace.
P Fe2O3 + 3CO → 2Fe + 3CO2
Q CaCO3 → CaO + CO2
Which type of reactions are P and Q?
P Q
A redox redox
B redox thermal decomposition
C thermal decomposition redox
D thermal decomposition thermal decomposition
13
© UCLES 2013 0620/11/O/N/13 [Turn over
29 Which row describes the uses of mild steel and stainless steel?
mild steel stainless steel
A car bodies, cutlery chemical plant, machinery
B car bodies, machinery chemical plant, cutlery
C chemical plant, cutlery car bodies, machinery
D chemical plant, machinery car bodies, cutlery
30 In which process is carbon dioxide not formed?
A burning of natural gas
B fermentation
C heating lime
D respiration 31 Farmers add calcium oxide (lime) and ammonium salts to their fields.
The compounds are not added at the same time because they react with each other.
Which gas is produced in this reaction?
A ammonia
B carbon dioxide
C hydrogen
D nitrogen 32 The diagrams show four uses of iron.
In which of these uses is the iron most likely to rust?
iron bucketelectroplated
with zinc
A
iron coredaluminium
electricity cables
B
iron hingeson a gate
C
paintediron fence
D
14
© UCLES 2013 0620/11/O/N/13
33 Which air pollutant is not made when coal burns in a power station?
A carbon monoxide
B lead compounds
C nitrogen oxides
D sulfur dioxide 34 In many countries river water is used for the washing of clothes.
The same water is not considered to be safe for drinking.
Why is it not safe for drinking?
A because river water contains dissolved salts
B because river water may contain harmful bacteria
C because river water may contain small particles of sand
D because river water may contain soap from washing clothes 35 The diagram shows a kiln used to heat limestone.
gas burners
productair
waste gases
limestone
What is the product and what waste gas is formed?
product waste gas
A lime, CaO carbon monoxide
B lime, CaO carbon dioxide
C slaked lime, Ca(OH)2 carbon monoxide
D slaked lime, Ca(OH)2 carbon dioxide
15
© UCLES 2013 0620/11/O/N/13 [Turn over
36 Three types of organic compound are alkanes, alkenes and alcohols.
Which structure does not belong to any of these three types of compound?
H C
H
H
C
H
H
C
O
O H H C
H
H
C
H
H
C
H
H
OH
H C
H
H
HC C
H
H
H
HC
H
H
A B
C D
C
H
H
C
H
H
37 The diagram shows some properties of two organic compounds X and Y.
reactswith
bromine
polymerises
X
usedas afuel
usedas a
solvent
Ysteamand a
catalyst
What are X and Y?
X Y
A ethane ethanoic acid
B ethane ethanol
C ethene ethanoic acid
D ethene ethanol
16
© UCLES 2013 0620/11/O/N/13
38 Petroleum is a mixture of hydrocarbons which can be separated into fractions using fractional distillation.
Which fraction is used as fuel in jet engines?
A bitumen
B gasoline
C kerosene
D naphtha 39 The diagram represents ethene.
C C
H
H
H
H
Which compound has chemical properties similar to those of ethene?
C CH H
H
H
H
A
H
C CH H
H
H
H
B
H
C
H
H
C CH
H
H
H
D
C
H
H
C CH H
H
H
C
O
H
H
17
© UCLES 2013 0620/11/O/N/13
40 A chemist carried out a cracking reaction on a hydrocarbon, X, and obtained two products, Y and Z.
H C
H
H
C
H
H
C
H
H
C
H
H
H H C
H
H
C
H
C
H
H
+X
Y Z
The chemist then wrote the following statements in his notebook.
1 A molecule of X has 7 carbon atoms.
2 Y is unsaturated.
3 Z will decolourise bromine water.
Which statements are correct?
A 3 only B 1 and 2 C 1 and 3 D 1, 2 and 3
18
© UCLES 2013 0620/11/O/N/13
BLANK PAGE
19
© UCLES 2013 0620/11/O/N/13
BLANK PAGE
20
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will be pleased to make amends at the earliest possible opportunity.
Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2013 0620/11/O/N/13
Gro
up
140
Ce
Cer
ium
58
141
PrP
rase
odym
ium
59
144
Nd
Neo
dym
ium
60
PmP
rom
ethi
um61
150
SmS
amar
ium
62
152
EuE
urop
ium
63
157
Gd
Gad
olin
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64
159
Tb Terb
ium
65
162
Dy
Dys
pros
ium
66
165
Ho
Hol
miu
m67
167
Er Erb
ium
68
169
Tm Thul
ium
69
173
YbY
tterb
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70
175
LuLu
tetiu
m71
232
Th Thor
ium
90
PaP
rota
ctin
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91
238 U
Ura
nium
92
Np
Nep
tuni
um93
PuP
luto
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94
Am
Am
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95
Cm
Cur
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96
Bk
Ber
keliu
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Cf
Cal
iforn
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98
EsE
inst
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Fm Ferm
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100
Md
Men
dele
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101
No
Nob
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m10
2
LrLa
wre
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m10
3
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ydro
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7 LiLi
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23 Na
Sod
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11
24 Mg
Mag
nesi
um12
40 Ca
Cal
cium
20
45 ScS
cand
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21
48 TiTi
tani
um22
51 VVa
nadi
um23
52 Cr
Chr
omiu
m24
55 Mn
Man
gane
se25
56 Fe Iron
26
59 Co
Cob
alt
27
59 Ni
Nic
kel
28
64 Cu
Cop
per
29
65 Zn Zinc
30
70 Ga
Gal
lium
31
27 Al
Alu
min
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13
11 B Bor
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12 CC
arbo
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14 NN
itrog
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16 OO
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19 FFl
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28 Si Sili
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31 PP
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32 S Sul
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Chl
orin
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40 Ar
Arg
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20 Ne
Neo
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4 He
Hel
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73 Ge
Ger
man
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75 As
Ars
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33
79 SeS
elen
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34
80 Br
Bro
min
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84 Kr
Kry
pton
36
39 KP
otas
sium
19
88 SrS
tront
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38
89 YY
ttriu
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91 ZrZi
rcon
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40
93 Nb
Nio
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41
96 Mo
Mol
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TcTe
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101
Ru
Rut
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103
Rh
Rho
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106
PdP
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46
108
Ag
Silv
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112
Cd
Cad
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115
In Indi
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119
Sn Tin
50
122
SbA
ntim
ony
51
128
TeTe
lluriu
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127 I
Iodi
ne53
131
Xe Xen
on54
137
Ba
Bar
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56
139
LaLa
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57
*
178
Hf
Haf
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72
181
TaTa
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Tung
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186
Re
Rhe
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75
190
Os
Osm
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76
192
Ir Iridi
um77
195 Pt
Pla
tinum
78
197
Au
Gol
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201
Hg
Mer
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204 Tl
Thal
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207
Pb Lead
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PoP
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At
Ast
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Rn
Rad
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FrFr
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This document consists of 18 printed pages and 2 blank pages.
IB13 11_0620_12/FP © UCLES 2013 [Turn over
*9656669434*
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education
CHEMISTRY 0620/12
Paper 1 Multiple Choice October/November 2013
45 Minutes Additional Materials: Multiple Choice Answer Sheet Soft clean eraser Soft pencil (type B or HB is recommended)
READ THESE INSTRUCTIONS FIRST
Write in soft pencil.
Do not use staples, paper clips, highlighters, glue or correction fluid.
Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless this has been done for you.
DO NOT WRITE IN ANY BARCODES.
There are forty questions on this paper. Answer all questions. For each question there are four possible answers A, B, C and D.
Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.
Read the instructions on the Answer Sheet very carefully.
Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
Any rough working should be done in this booklet.
A copy of the Periodic Table is printed on page 20.
Electronic calculators may be used.
2
© UCLES 2013 0620/12/O/N/13
1 An attempt was made to compress a gas and a solid using the apparatus shown.
piston
gas solid
Which substance would be compressed and what is the reason for this?
substance reason
A gas the gas particles are close together
B gas the gas particles are far apart
C solid the solid particles are close together
D solid the solid particles are far apart
2 A student measures the rate of two reactions.
In one reaction, there is a change in mass of the reactants during the reaction.
In the second reaction, there is a change in temperature during the reaction.
Which piece of apparatus would be essential in both experiments?
A balance
B clock
C pipette
D thermometer
3
© UCLES 2013 0620/12/O/N/13 [Turn over
3 Diagram 1 shows the paper chromatogram of substance X.
R
Y
X
diagram 1
Diagram 2 shows the cooling curve for substance Y.
0
147
0
temperature / °C
time
diagram 2
Which statement about X and Y is correct?
A X is a mixture and Y is a pure substance.
B X is a pure substance and Y is a mixture.
C X and Y are mixtures.
D X and Y are pure substances.
4 Which statements about a sodium atom, Na,23
11 are correct?
1 The number of protons and neutrons is the same.
2 The number of protons and electrons is the same.
3 The number of outer electrons is one.
A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only
4
© UCLES 2013 0620/12/O/N/13
5 The diagrams show the electron arrangements in the atoms of four elements.
Which element does not form a covalent bond?
e e
e e e
e e
e e
e e e e
e e e e
e e key
electron
nucleus
A B C D
e e
e e e e
e e
6 Rubidium is in Group I of the Periodic Table and bromine is in Group VII.
Rubidium reacts with bromine to form an ionic compound.
Which row shows the electron change taking place for rubidium and the correct formula of the rubidium ion?
electron change formula of ion formed
A electron gained Rb+
B electron gained Rb–
C electron lost Rb+
D electron lost Rb–
7 Element X has 7 protons.
Element Y has 8 more protons than X.
Which statement about element Y is correct?
A Y has more electron shells than X.
B Y has more electrons in its outer shell than X.
C Y is in a different group of the Periodic Table from X.
D Y is in the same period of the Periodic Table as X
5
© UCLES 2013 0620/12/O/N/13 [Turn over
8 The formulae of compounds W, X and Y are shown.
W CuSO4.5H2O
X MgSO4.7H2O
Y Cu(NO3)2.6H2O
Which statement is correct?
A W contains twice as many hydrogen atoms as oxygen atoms.
B X contains the most oxygen atoms.
C Y contains the most hydrogen atoms.
D Y contains the same number of hydrogen and oxygen atoms. 9 A solid mixture contains an ionic salt, X, and a covalent organic compound, Y.
Two students suggest methods of separating the mixture as shown.
method 1
method 2
shake withwater
X + Y
shake withethanol
X + Y
Which methods of separation are likely to work?
1 2
A � �
B � �
C � �
D � �
6
© UCLES 2013 0620/12/O/N/13
10 The diagram shows the circuit for electrolysing lead(II) bromide and sodium chloride to liberate the metal.
A
container forlead(II) bromide
container forsodium chloride
In what form are these salts electrolysed for liberating the metal?
lead(II) bromide sodium chloride
A concentrated solution concentrated solution
B concentrated solution molten
C molten concentrated solution
D molten molten
11 Which relative molecular mass, Mr, is not correct for the molecule given?
molecule Mr
A ammonia, NH3 17
B carbon dioxide, CO2 44
C methane, CH4 16
D oxygen, O2 16
7
© UCLES 2013 0620/12/O/N/13 [Turn over
12 When anhydrous copper(II) sulfate is added to water a solution is formed and heat is given out.
water
anhydrouscopper(II) sulfate
thermometer
Which row correctly shows the temperature change and the type of reaction taking place?
temperature change type of reaction
A decreases endothermic
B decreases exothermic
C increases endothermic
D increases exothermic
13 The diagram shows the electrolysis of concentrated aqueous sodium chloride.
+ –anode cathode
concentratedaqueous sodiumchloride and litmus
carbonrods
What is the colour of the litmus at each electrode after five minutes?
colour at anode colour at cathode
A blue red
B red blue
C red colourless
D colourless blue
8
© UCLES 2013 0620/12/O/N/13
14 Anhydrous copper(II) sulfate can be made by heating hydrated copper(II) sulfate.
CuSO4.5H2O → CuSO4 + 5H2O
What can be added to anhydrous copper(II) sulfate to turn it into hydrated copper(II) sulfate?
A concentrated sulfuric acid
B sodium hydroxide powder
C sulfur dioxide
D water 15 Which fuel does not produce carbon dioxide when it burns?
A coal
B hydrogen
C methane
D petrol 16 A student investigates the rate of reaction between zinc and an excess of sulfuric acid.
The graph shows the results of two experiments, X and Y.
0
X
Y
time0
volume ofhydrogen
Which change explains the difference between X and Y?
A A catalyst is added in Y.
B A lower temperature is used in Y.
C Larger pieces of zinc are used in Y.
D Less concentrated acid is used in Y.
9
© UCLES 2013 0620/12/O/N/13 [Turn over
17 Which are properties of an acid?
1 reacts with ammonium sulfate to form ammonia
2 turns red litmus blue
1 2
A � �
B � �
C � �
D � �
18 Which of the following are properties of the oxides of non-metals?
property 1 property 2
A acidic covalent
B acidic ionic
C basic covalent
D basic ionic
19 The reactions shown may occur in the air during a thunder storm.
N2 + O2 → 2NO
2NO + O2 → 2NO2
NO + O3 → NO2 + O2
Which row shows what happens to the reactant molecules in each of these reactions?
N2 NO O3
A oxidised oxidised oxidised
B oxidised oxidised reduced
C reduced reduced oxidised
D reduced reduced reduced
10
© UCLES 2013 0620/12/O/N/13
20 Calcium, on the left of Period 4 of the Periodic Table, is more metallic than bromine on the right of this period.
Why is this?
Calcium has
A fewer electrons.
B fewer protons.
C fewer full shells of electrons.
D fewer outer shell electrons. 21 Compound X is tested and the results are shown in the table.
test result
aqueous sodium hydroxide is
added, then heated gently
gas given off which turns damp
red litmus paper blue
dilute hydrochloric acid is added effervescence, gas given off
which turns limewater milky
Which ions are present in compound X?
A ammonium ions and carbonate ions
B ammonium ions and chloride ions
C calcium ions and carbonate ions
D calcium ions and chloride ions 22 Some properties of four elements W, X, Y and Z are listed.
1 W melts at 1410 °C and forms an acidic oxide.
2 X has a high density and is easily drawn into wires.
3 Y acts as a catalyst and its oxide reacts with acids.
4 Z is a red-brown solid used to make alloys.
Which of the elements are metals?
A 1 and 3 B 2, 3 and 4 C 2 and 3 only D 2 and 4 only
11
© UCLES 2013 0620/12/O/N/13 [Turn over
23 The diagram shows a light bulb.
filament
argon
Why is argon used instead of air in the light bulb?
A Argon is a good conductor of electricity.
B Argon is more reactive than air.
C The filament glows more brightly.
D The filament does not react with the argon.
24 An element has a melting point of 1084 °C and a density of 8.93 g / cm3. It’s oxide can be used as a catalyst.
In which position in the Periodic Table is the element found?
A B C
D
25 The diagrams show the labels of four bottles.
Which label is not correct?
A B C D
Bromine Br2
Harmful liquid.
Do not spill.
Iodine
I2
Danger Avoid breathing vapour
from the solid.
Potassium
K
Danger Store under water.
Sodium
Na
Danger Store under oil.
12
© UCLES 2013 0620/12/O/N/13
26 Equations P and Q represent two reactions which occur inside a blast furnace.
P Fe2O3 + 3CO → 2Fe + 3CO2
Q CaCO3 → CaO + CO2
Which type of reactions are P and Q?
P Q
A redox redox
B redox thermal decomposition
C thermal decomposition redox
D thermal decomposition thermal decomposition
27 Farmers add calcium oxide (lime) and ammonium salts to their fields.
The compounds are not added at the same time because they react with each other.
Which gas is produced in this reaction?
A ammonia
B carbon dioxide
C hydrogen
D nitrogen 28 Which row describes the uses of mild steel and stainless steel?
mild steel stainless steel
A car bodies, cutlery chemical plant, machinery
B car bodies, machinery chemical plant, cutlery
C chemical plant, cutlery car bodies, machinery
D chemical plant, machinery car bodies, cutlery
13
© UCLES 2013 0620/12/O/N/13 [Turn over
29 Reactions of three metals and their oxides are listed in the table.
metal reacts with cold water
metal oxide reacts with carbon
W no no
X no yes
Y yes no
What is the order of reactivity of the metals?
least reactive most reactive
A W X Y
B X W Y
C X Y W
D Y W X
30 The diagrams show four uses of iron.
In which of these uses is the iron most likely to rust?
iron bucketelectroplated
with zinc
A
iron coredaluminium
electricity cables
B
iron hingeson a gate
C
paintediron fence
D
31 In which process is carbon dioxide not formed?
A burning of natural gas
B fermentation
C heating lime
D respiration
14
© UCLES 2013 0620/12/O/N/13
32 M is a shiny silver metal. It has a melting point of 1455 °C. Many of its compounds are green.
What is metal M?
A aluminium
B copper
C mercury
D nickel 33 In many countries river water is used for the washing of clothes.
The same water is not considered to be safe for drinking.
Why is it not safe for drinking?
A because river water contains dissolved salts
B because river water may contain harmful bacteria
C because river water may contain small particles of sand
D because river water may contain soap from washing clothes
15
© UCLES 2013 0620/12/O/N/13 [Turn over
34 The diagram shows a kiln used to heat limestone.
gas burners
productair
waste gases
limestone
What is the product and what waste gas is formed?
product waste gas
A lime, CaO carbon monoxide
B lime, CaO carbon dioxide
C slaked lime, Ca(OH)2 carbon monoxide
D slaked lime, Ca(OH)2 carbon dioxide
35 Which air pollutant is not made when coal burns in a power station?
A carbon monoxide
B lead compounds
C nitrogen oxides
D sulfur dioxide
16
© UCLES 2013 0620/12/O/N/13
36 The diagram shows some properties of two organic compounds X and Y.
reactswith
bromine
polymerises
X
usedas afuel
usedas a
solvent
Ysteamand a
catalyst
What are X and Y?
X Y
A ethane ethanoic acid
B ethane ethanol
C ethene ethanoic acid
D ethene ethanol
37 Three types of organic compound are alkanes, alkenes and alcohols.
Which structure does not belong to any of these three types of compound?
H C
H
H
C
H
H
C
O
O H H C
H
H
C
H
H
C
H
H
OH
H C
H
H
HC C
H
H
H
HC
H
H
A B
C D
C
H
H
C
H
H
17
© UCLES 2013 0620/12/O/N/13
38 The diagram represents ethene.
C C
H
H
H
H
Which compound has chemical properties similar to those of ethene?
C CH H
H
H
H
A
H
C CH H
H
H
H
B
H
C
H
H
C CH
H
H
H
D
C
H
H
C CH H
H
H
C
O
H
H 39 Petroleum is a mixture of hydrocarbons which can be separated into fractions using fractional
distillation.
Which fraction is used as fuel in jet engines?
A bitumen
B gasoline
C kerosene
D naphtha 40 A chemist carried out a cracking reaction on a hydrocarbon, X, and obtained two products, Y
and Z.
H C
H
H
C
H
H
C
H
H
C
H
H
H H C
H
H
C
H
C
H
H
+X
Y Z
The chemist then wrote the following statements in his notebook.
1 A molecule of X has 7 carbon atoms.
2 Y is unsaturated.
3 Z will decolourise bromine water.
Which statements are correct?
A 3 only B 1 and 2 C 1 and 3 D 1, 2 and 3
18
© UCLES 2013 0620/12/O/N/13
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19
© UCLES 2013 0620/12/O/N/13
BLANK PAGE
20
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will be pleased to make amends at the earliest possible opportunity.
Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2013 0620/12/O/N/13
Gro
up
140
Ce
Cer
ium
58
141
PrP
rase
odym
ium
59
144
Nd
Neo
dym
ium
60
PmP
rom
ethi
um61
150
SmS
amar
ium
62
152
EuE
urop
ium
63
157
Gd
Gad
olin
ium
64
159
Tb Terb
ium
65
162
Dy
Dys
pros
ium
66
165
Ho
Hol
miu
m67
167
Er Erb
ium
68
169
Tm Thul
ium
69
173
YbY
tterb
ium
70
175
LuLu
tetiu
m71
232
Th Thor
ium
90
PaP
rota
ctin
ium
91
238 U
Ura
nium
92
Np
Nep
tuni
um93
PuP
luto
nium
94
Am
Am
eric
ium
95
Cm
Cur
ium
96
Bk
Ber
keliu
m97
Cf
Cal
iforn
ium
98
EsE
inst
eini
um99
Fm Ferm
ium
100
Md
Men
dele
vium
101
No
Nob
eliu
m10
2
LrLa
wre
nciu
m10
3
1 HH
ydro
gen
1
7 LiLi
thiu
m3
23 Na
Sod
ium
11
24 Mg
Mag
nesi
um12
40 Ca
Cal
cium
20
45 ScS
cand
ium
21
48 TiTi
tani
um22
51 VVa
nadi
um23
52 Cr
Chr
omiu
m24
55 Mn
Man
gane
se25
56 Fe Iron
26
59 Co
Cob
alt
27
59 Ni
Nic
kel
28
64 Cu
Cop
per
29
65 Zn Zinc
30
70 Ga
Gal
lium
31
27 Al
Alu
min
ium
13
11 B Bor
on5
12 CC
arbo
n6
14 NN
itrog
en7
16 OO
xyge
n8
19 FFl
uorin
e9
28 Si Sili
con
14
31 PP
hosp
horu
s15
32 S Sul
fur
16
35.5 Cl
Chl
orin
e17
40 Ar
Arg
on18
20 Ne
Neo
n10
4 He
Hel
ium
2
73 Ge
Ger
man
ium
32
75 As
Ars
enic
33
79 SeS
elen
ium
34
80 Br
Bro
min
e35
84 Kr
Kry
pton
36
39 KP
otas
sium
19
88 SrS
tront
ium
38
89 YY
ttriu
m39
91 ZrZi
rcon
ium
40
93 Nb
Nio
bium
41
96 Mo
Mol
ybde
num
42
TcTe
chne
tium
43
101
Ru
Rut
heni
um44
103
Rh
Rho
dium
45
106
PdP
alla
dium
46
108
Ag
Silv
er47
112
Cd
Cad
miu
m48
115
In Indi
um49
119
Sn Tin
50
122
SbA
ntim
ony
51
128
TeTe
lluriu
m52
127 I
Iodi
ne53
131
Xe Xen
on54
137
Ba
Bar
ium
56
139
LaLa
ntha
num
57
*
178
Hf
Haf
nium
72
181
TaTa
ntal
um73
184 W
Tung
sten
74
186
Re
Rhe
nium
75
190
Os
Osm
ium
76
192
Ir Iridi
um77
195 Pt
Pla
tinum
78
197
Au
Gol
d79
201
Hg
Mer
cury
80
204 Tl
Thal
lium
81
207
Pb Lead
82
209 Bi
Bis
mut
h83
PoP
olon
ium
84
At
Ast
atin
e85
Rn
Rad
on86
FrFr
anci
um87
227
Ac
Act
iniu
m89
9 Be
Ber
ylliu
m4
III
IIIIV
VV
IV
II0
85 Rb
Rub
idiu
m37
133
Cs
Cae
sium
55
226
Ra
Rad
ium
88
The
volu
me
of o
ne m
ole
of a
ny g
as is
24
dm3
at ro
om te
mpe
ratu
re a
nd p
ress
ure
(r.t.p
.).
a Xb
a =
rela
tive
atom
ic m
ass
X =
atom
ic s
ymbo
l
b =
prot
on (a
tom
ic) n
umbe
r
Key
* 58-
71 L
anth
anoi
d se
ries
90-1
03 A
ctin
oid
serie
s
DAT
A SH
EET
The
Perio
dic
Tabl
e of
the
Elem
ents
This document consists of 19 printed pages and 1 blank page.
IB13 11_0620_13/RP © UCLES 2013 [Turn over
*5450428188*
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education
CHEMISTRY 0620/13
Paper 1 Multiple Choice October/November 2013
45 Minutes Additional Materials: Multiple Choice Answer Sheet Soft clean eraser Soft pencil (type B or HB is recommended)
READ THESE INSTRUCTIONS FIRST
Write in soft pencil.
Do not use staples, paper clips, highlighters, glue or correction fluid.
Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless this has been done for you.
DO NOT WRITE IN ANY BARCODES.
There are forty questions on this paper. Answer all questions. For each question there are four possible answers A, B, C and D.
Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.
Read the instructions on the Answer Sheet very carefully.
Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
Any rough working should be done in this booklet.
A copy of the Periodic Table is printed on page 20.
Electronic calculators may be used.
2
© UCLES 2013 0620/13/O/N/13
1 A gas jar of bromine vapour and a gas jar of air are set up as shown in diagram 1.
The glass slide is removed. Diagram 2 shows the appearance of the gas jars after one hour.
diagram 1 diagram 2
brominevapour
mixture of airand bromine
air
glass slide
Which statement explains why the bromine and air mix together?
A Bromine is denser than air.
B Bromine is lighter than air.
C Bromine molecules moved upwards and molecules in air moved downwards.
D Molecules in bromine and air moved randomly. 2 The diagram shows a method for separating a substance that contains X and Y.
filter paper
X
Y
Which types of substance can be separated as shown?
A compounds
B elements
C mixtures
D molecules
3
© UCLES 2013 0620/13/O/N/13 [Turn over
3 Diagram 1 shows the paper chromatogram of substance X.
R
Y
X
diagram 1
Diagram 2 shows the cooling curve for substance Y.
0
147
0
temperature / °C
time
diagram 2
Which statement about X and Y is correct?
A X is a mixture and Y is a pure substance.
B X is a pure substance and Y is a mixture.
C X and Y are mixtures.
D X and Y are pure substances.
4
© UCLES 2013 0620/13/O/N/13
4 The atomic structures of four atoms are shown.
atom number of neutrons
number of protons
number of electrons
W 6 6 6
X 7 7 7
Y 8 6 6
Z 8 8 8
Which pair of atoms are isotopes?
A W and X B W and Y C X and Y D Y and Z 5 The diagram shows the structure of three particles, R, S and T.
3 p3 n
key
= electron
= neutron
= proton
= nucleus
e ee
e
n
p
R
3 p3 n
e e
S
3 p4 n
e ee
T
Which row describes these particles?
ions isotopes
A R S and T
B R and S T
C S R and T
D T R and S
6 Which statement about the bonding in a molecule of water is not correct?
A Both hydrogen and oxygen have a noble gas configuration of electrons.
B Each hydrogen shares its one electron with oxygen.
C Oxygen shares one of its own electrons with each hydrogen.
D Oxygen shares two of its own electrons with each hydrogen.
5
© UCLES 2013 0620/13/O/N/13 [Turn over
7 The electronic structures of atoms P and Q are shown.
P Q
P and Q react to form an ionic compound.
What is the formula of the compound?
A Q7P B QP C QP3 D QP7 8 A solid mixture contains an ionic salt, X, and a covalent organic compound, Y.
Two students suggest methods of separating the mixture as shown.
method 1
method 2
shake withwater
X + Y
shake withethanol
X + Y
Which methods of separation are likely to work?
1 2
A � �
B � �
C � �
D � �
6
© UCLES 2013 0620/13/O/N/13
9 Which relative molecular mass, Mr, is not correct for the molecule given?
molecule Mr
A ammonia, NH3 17
B carbon dioxide, CO2 44
C methane, CH4 16
D oxygen, O2 16
10 Two electrolysis experiments were carried out as shown in the diagram below.
The graphite electrodes are labelled 1-4.
molten sodium chloride
1 2 3 4
concentrated aqueoussodium chloride
+ +– –
Which row describes the products at the electrodes in these experiments?
electrode 1 electrode 2 electrode 3 electrode 4
A chlorine hydrogen chlorine hydrogen
B chlorine sodium chlorine hydrogen
C chlorine sodium hydrogen chlorine
D sodium chlorine sodium chlorine
7
© UCLES 2013 0620/13/O/N/13 [Turn over
11 One molten compound and two aqueous solutions were electrolysed.
The table gives the compounds electrolysed and the electrodes used.
substance electrolysed electrodes
1 concentrated hydrochloric acid carbon
2 concentrated sodium chloride platinum
3 molten lead bromide platinum
In which experiments is a gas evolved at the cathode?
A 1, 2 and 3 B 1 and 2 only C 1 only D 3 only 12 When ammonium nitrate is added to water the temperature of the water decreases.
The ammonium nitrate can be recovered by evaporating the water added.
Which explains these observations?
A The ammonium nitrate dissolves in the water and the process is endothermic.
B The ammonium nitrate reacts with the water and the process is endothermic.
C The ammonium nitrate dissolves in the water and the process is exothermic.
D The ammonium nitrate reacts with the water and the process is exothermic. 13 Which substance could not be used as a fuel to heat water in a boiler?
A ethanol
B hydrogen
C methane
D oxygen 14 Which substance is not a fossil fuel?
A coal B kerosene C gasoline D wood
8
© UCLES 2013 0620/13/O/N/13
15 A student investigates the rate of reaction between zinc and an excess of sulfuric acid.
The graph shows the results of two experiments, X and Y.
0
X
Y
time0
volume ofhydrogen
Which change explains the difference between X and Y?
A A catalyst is added in Y.
B A lower temperature is used in Y.
C Larger pieces of zinc are used in Y.
D Less concentrated acid is used in Y.
16 When green iron(II) sulfate is heated, it turns white and a colourless liquid is produced. When the liquid is put back into the white solid it changes back to green.
What type of reaction takes place and what is the name of the liquid?
type of reaction name of liquid
A redox sulfuric acid
B redox water
C reversible sulfuric acid
D reversible water
9
© UCLES 2013 0620/13/O/N/13 [Turn over
17 The reactions shown may occur in the air during a thunder storm.
N2 + O2 → 2NO
2NO + O2 → 2NO2
NO + O3 → NO2 + O2
Which row shows what happens to the reactant molecules in each of these reactions?
N2 NO O3
A oxidised oxidised oxidised
B oxidised oxidised reduced
C reduced reduced oxidised
D reduced reduced reduced
18 Which are properties of an acid?
1 reacts with ammonium sulfate to form ammonia
2 turns red litmus blue
1 2
A � �
B � �
C � �
D � �
19 Which of the following are properties of the oxides of non-metals?
property 1 property 2
A acidic covalent
B acidic ionic
C basic covalent
D basic ionic
10
© UCLES 2013 0620/13/O/N/13
20 The cations shown are identified by the colour of the precipitates formed when an excess of an aqueous solution of X is added.
cations present effect of adding an excess of
aqueous X
iron(II) (Fe2+) green precipitate
copper(II) (Cu2+) light blue precipitate
iron(III) (Fe3+) red-brown precipitate
What is X?
A ammonia
B limewater
C silver nitrate
D sodium hydroxide 21 Calcium, on the left of Period 4 of the Periodic Table, is more metallic than bromine on the right of
this period.
Why is this?
Calcium has
A fewer electrons.
B fewer protons.
C fewer full shells of electrons.
D fewer outer shell electrons. 22 The diagrams show the labels of four bottles.
Which label is not correct?
A B C D
Bromine Br2
Harmful liquid.
Do not spill.
Iodine
I2
Danger Avoid breathing vapour
from the solid.
Potassium
K
Danger Store under water.
Sodium
Na
Danger Store under oil.
11
© UCLES 2013 0620/13/O/N/13 [Turn over
23 An element has a melting point of 1084 °C and a density of 8.93 g / cm3. It’s oxide can be used as a catalyst.
In which position in the Periodic Table is the element found?
A B C
D
24 The diagram shows a light bulb.
filament
argon
Why is argon used instead of air in the light bulb?
A Argon is a good conductor of electricity.
B Argon is more reactive than air.
C The filament glows more brightly.
D The filament does not react with the argon. 25 Duralumin is an alloy. It contains aluminium, copper and magnesium.
It has many uses including the manufacture of cooking utensils and ships.
Which statement about duralumin and its properties is correct?
A It is a good conductor of electricity.
B It is brittle.
C It is soluble in water.
D The aluminium, copper and magnesium are chemically combined.
12
© UCLES 2013 0620/13/O/N/13
26 The list gives the order of some metals (and hydrogen) in the reactivity series.
Metal X is also included:
Most reactive K
Mg
Zn
(H)
X
Least reactive Cu
Which row correctly shows the properties of metal X?
reacts with dilute acids
oxide reduced by carbon
A no no
B no yes
C yes no
D yes yes
27 A new bicycle is being developed. Two different materials are used in its construction, both of which must be corrosion resistant.
Which two metals could be used?
A aluminium and mild steel
B aluminium and stainless steel
C mild steel and pure iron
D pure iron and stainless steel
13
© UCLES 2013 0620/13/O/N/13 [Turn over
28 Iron is extracted from hematite in the Blast Furnace.
waste gases
raw materials
firebrick lining
air
slag
molten iron
The hematite contains silica as an impurity. What reacts with this impurity to remove it?
A calcium oxide
B carbon
C carbon dioxide
D oxygen 29 In which process is carbon dioxide not formed?
A burning of natural gas
B fermentation
C heating lime
D respiration
14
© UCLES 2013 0620/13/O/N/13
30 Carbon dioxide is produced when
X reacts with ethanol.
Y reacts with sodium carbonate.
What are X and Y?
X Y
A H2 HCl
B H2 NaOH
C O2 HCl
D O2 NaOH
31 A sample of fertiliser is tested by warming it with aqueous sodium hydroxide.
A colourless gas is produced which turns red litmus paper blue.
Which element, essential for plant growth, must be present?
A nitrogen
B phosphorus
C potassium
D sulfur 32 Iron rusts. This process involves the ……1…… of iron. Rusting can be prevented by covering the
iron with grease or paint which stops ……2…… from reaching the surface of the iron.
Which words correctly complete gaps 1 and 2?
1 2
A oxidation nitrogen
B oxidation oxygen
C reduction nitrogen
D reduction oxygen
15
© UCLES 2013 0620/13/O/N/13 [Turn over
33 Oxides of nitrogen are given out from car exhausts.
Which row best shows why oxides of nitrogen are unwanted?
acidic toxic
A no no
B no yes
C yes no
D yes yes
34 Water is treated at a water works to make it fit to drink.
What is present in the water when it leaves the waterworks?
A bacteria only
B bacteria and insoluble substances
C chlorine only
D chlorine and soluble substances
16
© UCLES 2013 0620/13/O/N/13
35 The diagram shows a kiln used to heat limestone.
gas burners
productair
waste gases
limestone
What is the product and what waste gas is formed?
product waste gas
A lime, CaO carbon monoxide
B lime, CaO carbon dioxide
C slaked lime, Ca(OH)2 carbon monoxide
D slaked lime, Ca(OH)2 carbon dioxide
36 Molecule X is both an alkene and a carboxylic acid.
Which row describes X?
saturated –COOH present
A no no
B no yes
C yes no
D yes yes
37 Which hydrocarbon reacts with steam to produce ethanol?
A C2H4 B C2H6 C C3H6 D C3H8
17
© UCLES 2013 0620/13/O/N/13 [Turn over
38 Petroleum is a mixture of different hydrocarbons.
Which process is used to separate the petroleum into groups of similar hydrocarbons?
A combustion
B cracking
C fractional distillation
D reduction 39 Which row represents compounds in the same homologous series?
H C
H
H
C
H
H
C
H
H
H
H C
H
H
C
H
H
C
H
H
C
H
H
H
H C
H
H
C
H
H
C
H
H
H
H C
H
H
C
H
H
O H
H C
H
H
C
OH
H
C
H
H
H
C C
H
H
H
C
H
H
C
H
H
H
H C
H
H
C
H
H
H
H C
H
H
O
H
H
C H
H C
H
H
C
Br
H
C
H
H
H
H C
H
C
H
H
C
H
C
H
H
H
H C
H
H
C
O
O H
A
B
C
D
C C
H
H
H
C
H
H
C
H
H
H
H
H
18
© UCLES 2013 0620/13/O/N/13
40 The diagram shows a flow diagram.
petroleum
substance X
● burns with a yellow flame
● does not decolourise bromine water
substance Y
● decolourises bromine water
● undergoes addition polymerisation
Which type of organic compounds are X and Y?
substance X substance Y
A alcohol alkane
B alkane alkene
C alkene alkane
D alkane alcohol
19
© UCLES 2013 0620/13/O/N/13
BLANK PAGE
20
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will be pleased to make amends at the earliest possible opportunity.
Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2013 0620/13/O/N/13
Gro
up
140
Ce
Cer
ium
58
141
PrP
rase
odym
ium
59
144
Nd
Neo
dym
ium
60
PmP
rom
ethi
um61
150
SmS
amar
ium
62
152
EuE
urop
ium
63
157
Gd
Gad
olin
ium
64
159
Tb Terb
ium
65
162
Dy
Dys
pros
ium
66
165
Ho
Hol
miu
m67
167
Er Erb
ium
68
169
Tm Thul
ium
69
173
YbY
tterb
ium
70
175
LuLu
tetiu
m71
232
Th Thor
ium
90
PaP
rota
ctin
ium
91
238 U
Ura
nium
92
Np
Nep
tuni
um93
PuP
luto
nium
94
Am
Am
eric
ium
95
Cm
Cur
ium
96
Bk
Ber
keliu
m97
Cf
Cal
iforn
ium
98
EsE
inst
eini
um99
Fm Ferm
ium
100
Md
Men
dele
vium
101
No
Nob
eliu
m10
2
LrLa
wre
nciu
m10
3
1 HH
ydro
gen
1
7 LiLi
thiu
m3
23 Na
Sod
ium
11
24 Mg
Mag
nesi
um12
40 Ca
Cal
cium
20
45 ScS
cand
ium
21
48 TiTi
tani
um22
51 VVa
nadi
um23
52 Cr
Chr
omiu
m24
55 Mn
Man
gane
se25
56 Fe Iron
26
59 Co
Cob
alt
27
59 Ni
Nic
kel
28
64 Cu
Cop
per
29
65 Zn Zinc
30
70 Ga
Gal
lium
31
27 Al
Alu
min
ium
13
11 B Bor
on5
12 CC
arbo
n6
14 NN
itrog
en7
16 OO
xyge
n8
19 FFl
uorin
e9
28 Si Sili
con
14
31 PP
hosp
horu
s15
32 S Sul
fur
16
35.5 Cl
Chl
orin
e17
40 Ar
Arg
on18
20 Ne
Neo
n10
4 He
Hel
ium
2
73 Ge
Ger
man
ium
32
75 As
Ars
enic
33
79 SeS
elen
ium
34
80 Br
Bro
min
e35
84 Kr
Kry
pton
36
39 KP
otas
sium
19
88 SrS
tront
ium
38
89 YY
ttriu
m39
91 ZrZi
rcon
ium
40
93 Nb
Nio
bium
41
96 Mo
Mol
ybde
num
42
TcTe
chne
tium
43
101
Ru
Rut
heni
um44
103
Rh
Rho
dium
45
106
PdP
alla
dium
46
108
Ag
Silv
er47
112
Cd
Cad
miu
m48
115
In Indi
um49
119
Sn Tin
50
122
SbA
ntim
ony
51
128
TeTe
lluriu
m52
127 I
Iodi
ne53
131
Xe Xen
on54
137
Ba
Bar
ium
56
139
LaLa
ntha
num
57
*
178
Hf
Haf
nium
72
181
TaTa
ntal
um73
184 W
Tung
sten
74
186
Re
Rhe
nium
75
190
Os
Osm
ium
76
192
Ir Iridi
um77
195 Pt
Pla
tinum
78
197
Au
Gol
d79
201
Hg
Mer
cury
80
204 Tl
Thal
lium
81
207
Pb Lead
82
209 Bi
Bis
mut
h83
PoP
olon
ium
84
At
Ast
atin
e85
Rn
Rad
on86
FrFr
anci
um87
227
Ac
Act
iniu
m89
9 Be
Ber
ylliu
m4
III
IIIIV
VV
IV
II0
85 Rb
Rub
idiu
m37
133
Cs
Cae
sium
55
226
Ra
Rad
ium
88
The
volu
me
of o
ne m
ole
of a
ny g
as is
24
dm3
at ro
om te
mpe
ratu
re a
nd p
ress
ure
(r.t.p
.).
a Xb
a =
rela
tive
atom
ic m
ass
X =
atom
ic s
ymbo
l
b =
prot
on (a
tom
ic) n
umbe
r
Key
* 58-
71 L
anth
anoi
d se
ries
90-1
03 A
ctin
oid
serie
s
DAT
A SH
EET
The
Perio
dic
Tabl
e of
the
Elem
ents
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name in the spaces at the top of this page.Write in dark blue or black pen.You may need to use a pencil for any diagrams, graphs or rough working.Do not use staples, paper clips, highlighters, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.
Answer all questions.Electronic calculators may be used.A copy of the Periodic Table is printed on page 16.You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.
CHEMISTRY 0620/21
Paper 2 October/November 2013
1 hour 15 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONSInternational General Certifi cate of Secondary Education
This document consists of 14 printed pages and 2 blank pages.
[Turn overIB13 11_0620_21/3RP© UCLES 2013
*7249373810*
2
0620/21/O/N/13© UCLES 2013
ForExaminer’s
Use
1 (a) Choose from the list of elements below to answer the following questions.
calciumheliumiodinenickel
nitrogensodiumsulfur
Each element can be used once, more than once or not at all.
Which element:
(i) is an element present in most fertilisers, .................................................... [1]
(ii) is in Group VI of the Periodic Table, ........................................................... [1]
(iii) is in Period 5 of the Periodic Table, ............................................................ [1]
(iv) has a single electron shell containing two electrons, .................................. [1]
(v) is a transition element, ................................................................................ [1]
(vi) forms ions with a single negative charge? .................................................. [1]
(b) What is the meaning of the term element ?
...........................................................................................................................................
..................................................................................................................................... [1]
(c) Many of the elements in the Periodic Table have metallic properties. Describe three physical properties which are typical of most metals.
1. .......................................................................................................................................
2. .......................................................................................................................................
3. ................................................................................................................................. [3]
[Total: 10]
3
0620/21/O/N/13© UCLES 2013 [Turn over
ForExaminer’s
Use
2 Hydrogen chloride is an acidic gas.
(a) (i) Complete the dot and cross diagram to show the electronic structure of hydrogen chloride.
HCl
[2]
(ii) Is hydrogen chloride a covalent or an ionic compound? Give a reason for your answer.
.............................................................................................................................. [1]
(b) Hydrogen chloride reacts with water to form hydrochloric acid. Which one of the following is the most likely pH of hydrochloric acid? Put a ring around the correct answer.
pH 2 pH 7 pH 9 pH 14[1]
(c) Hydrochloric acid reacts with both metal oxides and carbonates.
(i) Complete the word equation for the reaction of hydrochloric acid with calcium carbonate.
hydrochloric + calcium → ...................... + ...................... + ...................... acid carbonate ...................... ...................... [3]
(ii) Complete the symbol equation for the reaction of magnesium oxide with hydrochloric acid. Name the salt which is formed.
MgO + ......HCl → MgCl 2 + H2O
name of salt ......................................................................................................... [2]
4
0620/21/O/N/13© UCLES 2013
ForExaminer’s
Use
(d) A student reacted magnesium with hydrochloric acid to fi nd out how concentration affects the rate of reaction. The magnesium was in excess. He measured the volume of hydrogen produced at various time intervals.
The graph shows his results.
0 50 100 150 200 250 300 350
50
40
30
20
10
0
volu
me
of h
ydro
gen
/ cm
3
time / seconds
(i) At what time had the reaction just fi nished?
.............................................................................................................................. [1]
(ii) What volume of hydrogen gas is given off during the fi rst 50 seconds of the reaction?
volume of hydrogen ........................... cm3 [1]
(iii) The student repeated the experiment. State two factors, apart from the concentration of hydrochloric acid, that should be
kept constant when repeating the experiment.
1. ................................................................................................................................
2. .......................................................................................................................... [2]
[Total: 13]
5
0620/21/O/N/13© UCLES 2013 [Turn over
ForExaminer’s
Use
3 Organic compounds can be put into groups called homologous series.
(a) Complete the following sentences about organic compounds and homologous series. Use words from the list below.
carbon chlorine different elements functional
hydrocarbon hydrogen oxide similar sulfur
Organic compounds usually contain atoms of ........................... and ........................... .
Each homologous series contains compounds with ................................. chemical
properties due to the presence of the same ................................. group. [4]
(b) Ethanol belongs to the alcohol homologous series.
(i) Draw the structure of ethanol, showing all atoms and bonds.
[2]
(ii) State the name of the two compounds formed when ethanol burns in excess air.
.......................................................... and .......................................................... [2]
6
0620/21/O/N/13© UCLES 2013
ForExaminer’s
Use
(c) Salicylic acid is used to make aspirin. The structure of salicylic acid is shown below.
C
C
C C
C C
O H
H H
H
O OC
H
H
(i) On this structure, put a ring around the carboxylic acid functional group. [1]
(ii) How many carbon atoms are there in one molecule of salicylic acid?
.............................................................................................................................. [1]
(iii) When making drugs and medicines, it is important that the chemicals used are pure. State one other area of everyday life where purity is important.
.............................................................................................................................. [1]
[Total: 11]
7
0620/21/O/N/13© UCLES 2013 [Turn over
ForExaminer’s
Use
4 The structures of diamond and graphite are shown below.
diamond graphite
= carbon atom
(a) Describe the similarities and differences between these structures.
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [4]
(b) Graphite burns in excess air to form carbon dioxide. Describe a test for carbon dioxide.
test ....................................................................................................................................
result ........................................................................................................................... [2]
(c) When graphite is burnt in a limited supply of air, carbon monoxide is formed. State one adverse effect of carbon monoxide on health.
..................................................................................................................................... [1]
(d) In the blast furnace for the production of iron, carbon monoxide reduces iron(III) oxide.
Fe2O3 + 3CO → 2Fe + 3CO2
How does this equation show that carbon monoxide is acting as a reducing agent?
..................................................................................................................................... [1]
(e) Iron(III) oxide and coke (carbon) are raw materials used in the production of iron. State the names of two other raw materials used in the blast furnace for the production
of iron.
1. .......................................................................................................................................
2. ................................................................................................................................. [2]
[Total: 10]
8
0620/21/O/N/13© UCLES 2013
ForExaminer’s
Use
5 Many plants contain coloured pigments. A student crushes some plant leaves in alcohol to extract the pigments. She then separates the pigments using the apparatus shown below.
(a) Write the correct labels in the boxes in the diagram above. [2]
(b) Draw an X on the diagram above to show where a drop of the pigment solution is placed at the start of the experiment. [1]
(c) After leaving the apparatus for half an hour, the pigments separated from each other. State the name given to this method of separating pigments.
..................................................................................................................................... [1]
(d) Some plants can absorb nickel from the ground. The nickel can then be extracted from the plants and purifi ed by electrolysis.
+ – rod ofpure nickel
electrolyte
rod ofimpure nickel
power supply
(i) Which one of the following is the most suitable electrolyte for this electrolysis. Tick one box.
aqueous copper(II) sulfate
aqueous nickel(II) sulfate
solid nickel(II) sulfate
water [1]
9
0620/21/O/N/13© UCLES 2013 [Turn over
ForExaminer’s
Use
(ii) Which one of the following elements is most likely to be formed at the negative electrode during this electrolysis?
Put a ring around the correct answer.
chlorine nickel sulfur oxygen[1]
(iii) The positive electrode is called the anode. State the name of the negative electrode.
.............................................................................................................................. [1]
(e) Electroplating is used to put a thin layer of one metal on top of another by electrolysis. Give two reasons for electroplating metals.
1. .......................................................................................................................................
2. ................................................................................................................................. [2]
(f) (i) Hydrated nickel(II) chloride is green in colour. When hydrated nickel(II) chloride is heated gently, it changes colour from green to
white. Complete the symbol equation for this reaction.
NiCl 2.6H2O(s) NiCl 2(s) + .................... hydrated nickel(II) chloride [1]
(ii) What does the sign mean?
.............................................................................................................................. [1]
(iii) How can you obtain a sample of green nickel(II) chloride starting with white nickel(II) chloride?
.............................................................................................................................. [1]
[Total: 12]
10
0620/21/O/N/13© UCLES 2013
ForExaminer’s
Use
6 The diagram shows a kettle of boiling water.
kettlewater vapour
water droplets
As the water vapour cools it turns back to water droplets.
(a) Describe this change of state in terms of the kinetic particle theory. In your answer, include
● the difference in the closeness of the water molecules as the water vapour changes to water,
● the difference in the motion of the water molecules as the water vapour changes to water.
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [4]
(b) Water is a common solvent in the laboratory.
(i) What is meant by the term solvent ?
.............................................................................................................................. [1]
(ii) State the name of the solvent whose formula is C2H5OH.
.............................................................................................................................. [1]
(c) When ammonium chloride dissolves in water the temperature of the solution falls. State the name of the energy change which results in the temperature falling.
..................................................................................................................................... [1]
11
0620/21/O/N/13© UCLES 2013 [Turn over
ForExaminer’s
Use
(d) Which one of the following conducts electricity. Tick one box.
aqueous ammonium chloride
solid ammonium chloride
ammonia gas
chlorine gas
[1]
(e) (i) Complete the symbol equation for the reaction of lithium with water to form lithium hydroxide and hydrogen.
2Li + .....H2O → 2.......... + H2[2]
(ii) When 14 g of lithium react with water, 4 g of hydrogen are formed. Calculate the mass of hydrogen formed when 70 g of lithium react with water.
[1]
[Total: 11]
12
0620/21/O/N/13© UCLES 2013
ForExaminer’s
Use
7 The table shows some properties of seven different substances.
substance density/ g per cm3
relative strength
relative electrical conductivity
relative thermal
conductivity
aluminium 2.7 15 42 200.0
ceramic 2.5 15 does not conduct 1.6
copper 8.9 20 63 385.0
iron 7.9 25 11 80.0
lead 11.4 15 5 38.0
poly(ethene) 0.9 1 does not conduct 0.3
steel 7.8 90 2 25.0
(a) Use the information in this table to answer the following questions.
(i) Which substance is the best conductor of heat?
.............................................................................................................................. [1]
(ii) Suggest why copper is preferred to iron for electrical wiring in houses.
.............................................................................................................................. [1]
(iii) What property of ceramic makes it a good electrical insulator?
.............................................................................................................................. [1]
(iv) Which pure metal in the table conducts electricity least well?
.............................................................................................................................. [1]
(v) Suggest why steel rather than iron is used in making machinery.
.............................................................................................................................. [1]
(vi) Which metal in the table is the most dense?
.............................................................................................................................. [1]
(b) A solution of a metal salt reacts with aqueous sodium hydroxide to form a white precipitate. The white precipitate is soluble in excess aqueous sodium hydroxide.
(i) Which one of the following ions is most likely to be present in the salt? Put a ring around the correct answer.
calcium copper(II) iron(II) zinc[1]
(ii) State the name of the white precipitate.
.............................................................................................................................. [1]
13
0620/21/O/N/13© UCLES 2013 [Turn over
ForExaminer’s
Use
(c) Copper(II) chloride can be made by the action of hydrochloric acid on copper(II) oxide. Put the statements, A, B, C and D, about this preparation in the correct order.
A Leave the saturated solution to crystallise. B Filter the solution to remove excess copper(II) oxide. C Add excess copper(II) oxide to hydrochloric acid and warm. D Evaporate the fi ltrate to the crystallisation point.
..................................................................................................................................... [1]
(d) The structure of copper(II) chloride is shown below.
Cu2+
Cu2+
Cu2+Cu2+
Cl – Cl –
Cl – Cl –
Cl – Cl –
Cu2+
Cu2+
Cl – Cl –
Cl – Cl –
Cl – Cl –
Write the simplest formula for copper(II) chloride.
..................................................................................................................................... [1]
(e) Suggest the product formed at each electrode when molten copper(II) chloride is electrolysed.
at the positive electrode ....................................................................................................
at the negative electrode ............................................................................................ [2]
(f) When copper(II) chloride is heated strongly, a gas is given off. The gas is green in colour and bleaches litmus paper. State the name of this gas.
..................................................................................................................................... [1]
[Total: 13]
14
0620/21/O/N/13
BLANK PAGE
© UCLES 2013
15
0620/21/O/N/13
BLANK PAGE
© UCLES 2013
16
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Everyreasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included the publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
0620/21/O/N/13© UCLES 2013
Gro
up
140
Ce
Cer
ium
58
141
PrP
rase
odym
ium
59
144
Nd
Neo
dym
ium
60
PmP
rom
ethi
um61
150
SmS
amar
ium
62
152
EuE
urop
ium
63
157
Gd
Gad
olin
ium
64
159
Tb Terb
ium
65
162
Dy
Dys
pros
ium
66
165
Ho
Hol
miu
m67
167
Er Erb
ium
68
169
Tm Thul
ium
69
173
YbY
tterb
ium
70
175
LuLu
tetiu
m71
232
Th Thor
ium
90
PaP
rota
ctin
ium
91
238 U
Ura
nium
92
Np
Nep
tuni
um93
PuP
luto
nium
94
Am
Am
eric
ium
95
Cm
Cur
ium
96
Bk
Ber
keliu
m97
Cf
Cal
iforn
ium
98
EsE
inst
eini
um99
Fm Ferm
ium
100
Md
Men
dele
vium
101
No
Nob
eliu
m10
2
LrLa
wre
nciu
m10
3
1 HH
ydro
gen
1
7 LiLi
thiu
m3
23 Na
Sod
ium
11
24 Mg
Mag
nesi
um12
40 Ca
Cal
cium
20
45 ScS
cand
ium
21
48 TiTi
tani
um22
51 VVa
nadi
um23
52 Cr
Chr
omiu
m24
55 Mn
Man
gane
se25
56 Fe Iron
26
59 Co
Cob
alt
27
59 Ni
Nic
kel
28
64 Cu
Cop
per
29
65 Zn Zinc
30
70 Ga
Gal
lium
31
27 Al
Alu
min
ium
13
11 B Bor
on5
12 CC
arbo
n6
14 NN
itrog
en7
16 OO
xyge
n8
19 FFl
uorin
e9
28 Si Sili
con
14
31 PP
hosp
horu
s15
32 S Sul
fur
16
35.5 Cl
Chl
orin
e17
40 Ar
Arg
on18
20 Ne
Neo
n10
4 He
Hel
ium
2
73 Ge
Ger
man
ium
32
75 As
Ars
enic
33
79 SeS
elen
ium
34
80 Br
Bro
min
e35
84 Kr
Kry
pton
36
39 KP
otas
sium
19
88 SrS
tront
ium
38
89 YY
ttriu
m39
91 ZrZi
rcon
ium
40
93 Nb
Nio
bium
41
96 Mo
Mol
ybde
num
42
TcTe
chne
tium
43
101
Ru
Rut
heni
um44
103
Rh
Rho
dium
45
106
PdP
alla
dium
46
108
Ag
Silv
er47
112
Cd
Cad
miu
m48
115
In Indi
um49
119
Sn Tin
50
122
SbA
ntim
ony
51
128
TeTe
lluriu
m52
127 I
Iodi
ne53
131
Xe Xen
on54
137
Ba
Bar
ium
56
139
LaLa
ntha
num
57
*
178
Hf
Haf
nium
72
181
TaTa
ntal
um73
184 W
Tung
sten
74
186
Re
Rhe
nium
75
190
Os
Osm
ium
76
192
Ir Iridi
um77
195 Pt
Pla
tinum
78
197
Au
Gol
d79
201
Hg
Mer
cury
80
204 Tl
Thal
lium
81
207
Pb Lead
82
209 Bi
Bis
mut
h83
PoP
olon
ium
84
At
Ast
atin
e85
Rn
Rad
on86
FrFr
anci
um87
227
Ac
Act
iniu
m89
9 Be
Ber
ylliu
m4
III
IIIIV
VV
IV
II0
85 Rb
Rub
idiu
m37
133
Cs
Cae
sium
55
226
Ra
Rad
ium
88
The
volu
me
of o
ne m
ole
of a
ny g
as is
24
dm3
at ro
om te
mpe
ratu
re a
nd p
ress
ure
(r.t.p
.).
a Xb
a =
rela
tive
atom
ic m
ass
X =
atom
ic s
ymbo
l
b =
prot
on (a
tom
ic) n
umbe
r
Key
* 58-
71 L
anth
anoi
d se
ries
90-1
03 A
ctin
oid
serie
s
DAT
A SH
EET
The
Perio
dic
Tabl
e of
the
Elem
ents
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name in the spaces at the top of this page.Write in dark blue or black pen.You may need to use a pencil for any diagrams, graphs or rough working.Do not use staples, paper clips, highlighters, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.
Answer all questions.Electronic calculators may be used.A copy of the Periodic Table is printed on page 16.You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.
CHEMISTRY 0620/22
Paper 2 October/November 2013
1 hour 15 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONSInternational General Certifi cate of Secondary Education
This document consists of 15 printed pages and 1 blank page.
[Turn overIB13 11_0620_22/2RP© UCLES 2013
*5048513202*
2
0620/22/O/N/13
BLANK PAGE
© UCLES 2013
3
0620/22/O/N/13© UCLES 2013 [Turn over
ForExaminer’s
Use
1 (a) Choose from the list of compounds below to answer the following questions.
ammoniaammonium chloridecalcium carbonate
calcium oxidecopper(II) sulfate
ethaneiron(II) chloride
methanewater
Each compound can be used once, more than once or not at all.
Which compound:
(i) is an alkaline gas, ................................................................................... [1]
(ii) is a gas contributing to climate change, ................................................. [1]
(iii) is a salt containing only non-metals, ....................................................... [1]
(iv) turns blue cobalt chloride paper pink, ..................................................... [1]
(v) reacts with an acid to release carbon dioxide, ........................................ [1]
(vi) gives a light blue precipitate when aqueous sodium hydroxide is added to a solution of its aqueous ions? ................................................................................ [1]
(b) What is the meaning of the term compound ?
...........................................................................................................................................
..................................................................................................................................... [1]
(c) Complete the following symbol equation for the complete combustion of methane in oxygen.
CH4 + .......O2 → .................. + 2H2O[2]
[Total: 9]
4
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2 (a) The table describes the reactivity of some metals with hydrochloric acid.
metal observations
calcium Many bubbles produced. Reaction mixture may boil.
magnesium Steady stream of bubbles produced. Reaction mixture gets hot.
sodium Many bubbles produced. May explode.
zinc Slow stream of bubbles produced. Reaction mixture rises slightly in temperature.
Put these metals in order of their reactivity.
least reactive most reactive
[2]
(b) Complete the word equation for the reaction of magnesium with hydrochloric acid.
magnesium + hydrochloric acid → ............................ + ............................
............................ [2]
(c) When magnesium reacts with hydrochloric acid, magnesium atoms lose electrons. What type of magnesium particle is formed? Put a ring around the correct answer.
covalent ion molecule proton[1]
(d) Complete the diagram to show the electronic structure of a sodium atom.
Na
[2]
5
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(e) A student added large lumps of zinc to 20 cm3 of 2 mol / dm3 hydrochloric acid. She carried out the reaction at 15 °C. She measured the volume of gas given off at various time intervals.
(i) Draw a labelled diagram of the apparatus she could use for this experiment.
[3]
(ii) Describe three different things she could do to increase the rate of this reaction.
1. ................................................................................................................................
2. ................................................................................................................................
3. .......................................................................................................................... [3]
[Total: 13]
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3 The diagram below shows the apparatus which can be used to obtain pure water fromsea-water.
heat
sea-water
pure water
(a) State the name of this process.
..................................................................................................................................... [1]
(b) Label the boxes on the diagram above with the correct names of the pieces of apparatus shown. [3]
(c) Complete the following sentences using words from the list below.
boils condenses cools freezes
higher lower melts
Water has a ............................. boiling point than salt. When a solution of salt is heated
strongly, the water ............................. and escapes as steam. When the steam cools, it
............................. back to liquid water. [3]
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(d) The table shows the concentration of the seven most abundant compounds in sea-water.
compound ions present concentrationin g / m3
calcium carbonate Ca2+ and CO32– 100
calcium sulfate Ca2+ and SO42– 1 800
magnesium chloride Mg2+ and Cl – 6 800
magnesium sulfate 5 700
potassium bromide K+ and Br – 100
potassium chloride K+ and Cl – 800
sodium chloride Na+ and Cl – 28 000
(i) Which negative ion is present in the greatest concentration in sea-water?
.............................................................................................................................. [1]
(ii) Which positive ion is present in the lowest concentration in sea-water? .............................................................................................................................. [1]
(iii) Write the formulae of the two ions present in magnesium sulfate.
.............................................................................................................................. [2]
[Total: 11]
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4 (a) Match the compounds on the left with the statements on the right. The fi rst one has been done for you.
butane
poly(ethene)
ethene
methane
ethanoic acid
a hydrocarbon containingfour carbon atoms
it decolourisesbromine water
it is the main constituentof natural gas
it contains a –COOHfunctional group
it has a very long chainof carbon atoms
[4]
(b) Methane and ethene are hydrocarbons.
(i) What is meant by the term hydrocarbon ?
.............................................................................................................................. [1]
(ii) The structure of ethene is shown below.
C C
H
H
H
H
Use this structure to explain why ethene is an unsaturated hydrocarbon.
.............................................................................................................................. [1]
(c) Molecules of ethene react together at high temperature and pressure to form poly(ethene).
Which one of the following words best describes the molecules of ethene in this reaction? Put a ring around the correct answer.
acids alkanes monomers polymers[1]
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(d) Ethanoic acid can be made by the oxidation of ethanol.
(i) What is meant by the term oxidation ?
.............................................................................................................................. [1]
(ii) Ethanol can be made by fermentation. Complete the word equation for fermentation.
yeast.......................... → .......................... + ethanol
.......................... [2]
[Total: 10]
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5 (a) Explain why metals are often used in the form of alloys. In your answer, write about
● the structure of an alloy, ● why alloys are often more useful than pure metals.
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [3]
(b) Iron is a transition element.
(i) Which two of the following statements about iron are correct? Tick two boxes.
A freshly-cut surface of iron is green in colour.
Iron exists in only one oxidation state in its compounds.
Iron has a high density.
Iron has a giant covalent structure.
Iron has a high melting point. [2]
(ii) Describe one method of rust prevention and explain how it works.
method .......................................................................................................................
how this works ...........................................................................................................
.............................................................................................................................. [2]
(c) Iron is used as a catalyst in the Haber process for making ammonia.
(i) What does the term catalyst mean?
.............................................................................................................................. [1]
(ii) Describe a test for ammonia.
test .............................................................................................................................
result .................................................................................................................... [2]
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(iii) Ammonia is used to make fertilisers. Explain why farmers need to add fertilisers to the soil.
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [2]
[Total: 12]
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6 (a) Garlic is a vegetable that is often used in cooking. It has a strong smell. A student is cutting up garlic in the kitchen.
After a time, the smell of the garlic travels all over the house even though there are no currents of air.
Use the kinetic particle theory to explain why the smell of garlic travels all over the house.
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [3]
(b) The smell of garlic is due to a compound containing sulfur. The structure of this compound (compound A) is shown below.
CH2 CH — CH2 — S — S — CH2 — CH CH2
compound A
(i) Write the molecular formula for this compound.
.............................................................................................................................. [1]
(ii) Another organic sulfur compound (compound B) is shown below.
CH2H2C
C2H5
S
CHC
compound B
By comparing the formulae of compound A and compound B, how can you tell that compound A has the higher relative molecular mass?
You are not required to do any mathematical calculations.
....................................................................................................................................
.............................................................................................................................. [2]
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(c) An isotope of sulfur has a nucleon number of 34 and an atomic number of 16.
(i) How many neutrons are there in one atom of this isotope of sulfur?
.............................................................................................................................. [1]
(ii) What is meant by the terms
isotope, ......................................................................................................................
.............................................................................................................................. [1]
nucleon number ? ................................................................................................ [1]
(iii) Some fuels contain sulfur as a contaminating substance. Complete the following sentences using words from the list below.
coal dioxide hydrogen monoxide
nitrogen oxidised reduced water
Fuels such as ........................... contain sulfur.
When these fuels burn, the sulfur is ........................... to sulfur ........................... .
This reacts with ........................... in the atmosphere to form an acidic solution. [4]
(iv) Describe and explain the effect of acid rain on buildings made of limestone.
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [2]
[Total: 15]
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7 The diagram shows a kiln for making lime (calcium oxide) from limestone (calcium carbonate).
A
B
D
C
brick lime kiln
(a) (i) Which letter on the diagram above shows
where the limestone is added, ...................................................................................
where the waste gases exit from the kiln? ........................................................... [2]
(ii) Complete the symbol equation for the decomposition of limestone.
CaCO3 → CaO + .............[1]
(iii) When 50 g of calcium carbonate is decomposed, 28 g of calcium oxide is formed. Calculate the minimum mass of calcium carbonate needed to produce 8.4 g of
calcium oxide.
[1]
(b) The table below shows the temperatures at which some Group II carbonates decompose.
Group II carbonate temperature at which Group IIcarbonates decompose / °C
beryllium carbonate 100
magnesium carbonate 350
calcium carbonate 900
(i) Describe the pattern in the ease of decomposition of Group II carbonates.
.............................................................................................................................. [1]
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(ii) Predict the decomposition temperature of barium carbonate.
......................... °C [1]
(c) Lime is calcium oxide.
(i) State one use of lime.
.............................................................................................................................. [1]
(ii) What type of oxide is calcium oxide?
.............................................................................................................................. [1]
(iii) Calculate the relative formula mass of calcium oxide. Use your Periodic Table to help you.
[1]
(d) Calcium is extracted from its compounds by electrolysis. Suggest why calcium is extracted by electrolysis rather than by reduction with carbon.
..................................................................................................................................... [1]
[Total: 10]
16
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Everyreasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included the publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
0620/22/O/N/13© UCLES 2013
Gro
up
140
Ce
Cer
ium
58
141
PrP
rase
odym
ium
59
144
Nd
Neo
dym
ium
60
PmP
rom
ethi
um61
150
SmS
amar
ium
62
152
EuE
urop
ium
63
157
Gd
Gad
olin
ium
64
159
Tb Terb
ium
65
162
Dy
Dys
pros
ium
66
165
Ho
Hol
miu
m67
167
Er Erb
ium
68
169
Tm Thul
ium
69
173
YbY
tterb
ium
70
175
LuLu
tetiu
m71
232
Th Thor
ium
90
PaP
rota
ctin
ium
91
238 U
Ura
nium
92
Np
Nep
tuni
um93
PuP
luto
nium
94
Am
Am
eric
ium
95
Cm
Cur
ium
96
Bk
Ber
keliu
m97
Cf
Cal
iforn
ium
98
EsE
inst
eini
um99
Fm Ferm
ium
100
Md
Men
dele
vium
101
No
Nob
eliu
m10
2
LrLa
wre
nciu
m10
3
1 HH
ydro
gen
1
7 LiLi
thiu
m3
23 Na
Sod
ium
11
24 Mg
Mag
nesi
um12
40 Ca
Cal
cium
20
45 ScS
cand
ium
21
48 TiTi
tani
um22
51 VVa
nadi
um23
52 Cr
Chr
omiu
m24
55 Mn
Man
gane
se25
56 Fe Iron
26
59 Co
Cob
alt
27
59 Ni
Nic
kel
28
64 Cu
Cop
per
29
65 Zn Zinc
30
70 Ga
Gal
lium
31
27 Al
Alu
min
ium
13
11 B Bor
on5
12 CC
arbo
n6
14 NN
itrog
en7
16 OO
xyge
n8
19 FFl
uorin
e9
28 Si Sili
con
14
31 PP
hosp
horu
s15
32 S Sul
fur
16
35.5 Cl
Chl
orin
e17
40 Ar
Arg
on18
20 Ne
Neo
n10
4 He
Hel
ium
2
73 Ge
Ger
man
ium
32
75 As
Ars
enic
33
79 SeS
elen
ium
34
80 Br
Bro
min
e35
84 Kr
Kry
pton
36
39 KP
otas
sium
19
88 SrS
tront
ium
38
89 YY
ttriu
m39
91 ZrZi
rcon
ium
40
93 Nb
Nio
bium
41
96 Mo
Mol
ybde
num
42
TcTe
chne
tium
43
101
Ru
Rut
heni
um44
103
Rh
Rho
dium
45
106
PdP
alla
dium
46
108
Ag
Silv
er47
112
Cd
Cad
miu
m48
115
In Indi
um49
119
Sn Tin
50
122
SbA
ntim
ony
51
128
TeTe
lluriu
m52
127 I
Iodi
ne53
131
Xe Xen
on54
137
Ba
Bar
ium
56
139
LaLa
ntha
num
57
*
178
Hf
Haf
nium
72
181
TaTa
ntal
um73
184 W
Tung
sten
74
186
Re
Rhe
nium
75
190
Os
Osm
ium
76
192
Ir Iridi
um77
195 Pt
Pla
tinum
78
197
Au
Gol
d79
201
Hg
Mer
cury
80
204 Tl
Thal
lium
81
207
Pb Lead
82
209 Bi
Bis
mut
h83
PoP
olon
ium
84
At
Ast
atin
e85
Rn
Rad
on86
FrFr
anci
um87
227
Ac
Act
iniu
m89
9 Be
Ber
ylliu
m4
III
IIIIV
VV
IV
II0
85 Rb
Rub
idiu
m37
133
Cs
Cae
sium
55
226
Ra
Rad
ium
88
The
volu
me
of o
ne m
ole
of a
ny g
as is
24
dm3
at ro
om te
mpe
ratu
re a
nd p
ress
ure
(r.t.p
.).
a Xb
a =
rela
tive
atom
ic m
ass
X =
atom
ic s
ymbo
l
b =
prot
on (a
tom
ic) n
umbe
r
Key
* 58-
71 L
anth
anoi
d se
ries
90-1
03 A
ctin
oid
serie
s
DAT
A SH
EET
The
Perio
dic
Tabl
e of
the
Elem
ents
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name in the spaces at the top of this page.Write in dark blue or black pen.You may need to use a pencil for any diagrams, graphs or rough working.Do not use staples, paper clips, highlighters, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.
Answer all questions.Electronic calculators may be used.A copy of the Periodic Table is printed on page 16.You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.
CHEMISTRY 0620/23
Paper 2 October/November 2013
1 hour 15 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONSInternational General Certifi cate of Secondary Education
This document consists of 15 printed pages and 1 blank page.
[Turn overIB13 11_0620_23/2RP© UCLES 2013
*3407475716*
2
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1 (a) Choose from the list of metals below to answer the following questions.
aluminiumbariumcalciumironlithiumsilver
Each metal can be used once, more than once or not at all.
(i) Which metal has an atom with three electrons in its outer electron shell?
.............................................................................................................................. [1]
(ii) Which two metals are in the same Period of the Periodic Table?
.......................................................... and .......................................................... [1]
(iii) Which metal has an atom with three protons in its nucleus?
.............................................................................................................................. [1]
(iv) Which metal has a nitrate which is used to test for halide ions?
.............................................................................................................................. [1]
(v) Which metal is used in food containers because of its resistance to corrosion?
.............................................................................................................................. [1]
(b) Describe two chemical properties of iron.
1. .......................................................................................................................................
2. ................................................................................................................................. [2]
(c) Describe briefl y how iron from the blast furnace is made into steel.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
[Total: 9]
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2 Helium is in Group 0 of the Periodic Table.
(a) Describe the structure of a helium atom. Use your Periodic Table to help you. In your answer, include
● the type and number of subatomic particles present, ● the position of these particles in the atom, ● the relative charges on the particles.
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [5]
(b) Give one use of helium.
..................................................................................................................................... [1]
(c) Some elements in Group 0 can form compounds with fl uorine and oxygen. The structure of one of these compounds is shown below.
XeFF
FO
F
Calculate the relative molecular mass of this compound. Use your Periodic Table to help you. You must show all your working.
[2]
(d) Fluorine is a diatomic molecule. It melts at –220 °C and boils at –188 °C.
(i) What is the physical state of fl uorine
at room temperature, .................................................................................................
at –200 °C? .......................................................................................................... [2]
(ii) What is meant by the term diatomic ?
.............................................................................................................................. [1]
[Total: 11]
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3 This question is about calcium and some calcium compounds.
(a) Calcium is in Group II of the Periodic Table. Complete the diagram below to show the electronic structure of calcium.
Ca
[2]
(b) Calcium reacts with hydrochloric acid to form a salt with the formula CaCl 2. State the name of this salt.
..................................................................................................................................... [1]
(c) Calcium carbonate reacts with hydrochloric acid. The course of this reaction can be followed by measuring the volume of carbon dioxide
given off at various time intervals. The graph below shows the results obtained from an experiment using 0.15 g of calcium
carbonate in small pieces.
0 50 100 150 200
time / seconds
250 300 350 400
volu
me
of c
arbo
n di
oxid
e / c
m3
50
40
30
20
10
0
5
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(i) What volume of gas is given off in the fi rst 75 seconds of the reaction?
.............................................................................................................................. [1]
(ii) On the grid opposite, sketch the line you would expect for the same reaction using large pieces of calcium carbonate. Assume that the mass of the calcium carbonate and all other conditions remain the same. [2]
(iii) What would happen to the rate of this reaction if:
the temperature is increased,
....................................................................................................................................
the concentration of hydrochloric acid is decreased?
.............................................................................................................................. [2]
(d) When calcium carbonate is heated at high temperatures, calcium oxide and carbon dioxide are formed.
(i) Which one of the following words best describes this reaction? Put a ring around the correct answer.
combustion decomposition exothermic reduction[1]
(ii) Describe a test for carbon dioxide.
test .............................................................................................................................
result .................................................................................................................... [2]
(e) Calcium oxide can be used to neutralise acidic industrial waste.
(i) Complete the word equation for the reaction of calcium oxide with nitric acid.
calcium oxide + nitric acid → ........................ + ........................
........................ [2]
(ii) State one other use of calcium oxide.
.............................................................................................................................. [1]
(iii) When calcium oxide reacts with water, heat is given off. State the name given to a chemical reaction which gives off heat.
.............................................................................................................................. [1]
[Total: 15]
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4 The diagram shows how a liquid alkane can be cracked in a school laboratory to form a mixture of gaseous and liquid hydrocarbons.
water
catalyst(aluminium oxide granules)
liquid alkane(absorbed in mineral wool)
(a) What piece of apparatus is missing from the diagram?
..................................................................................................................................... [1]
(b) On the diagram above, put an X to show where the gas is collected. [1]
(c) What is the purpose of the catalyst?
..................................................................................................................................... [1]
(d) Complete the equation to show the cracking of dodecane, C12H26, to form octane and one other substance.
C12H26 → C8H18 + .................[1]
(e) Cracking produces a mixture of shorter-chain alkanes and alkenes.
(i) Describe what you would observe when a few drops of bromine water are added to an alkene.
.............................................................................................................................. [1]
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(ii) Which one of the following compounds, A, B, C or D, is formed when bromine water reacts with ethene?
C
H H
C
A
Br Br
CH
H H
C H
B
Br Br
CH C H
OH OH
OH OH
C
C C
D
Br Br
BrBr
Br Br
.............................................................................................................................. [1]
(iii) Poly(ethene) is made by combining ethene monomers. Which one of the following describes this reaction? Tick one box.
decomposition
neutralisation
oxidation
polymerisation [1]
(f) Many alkanes found in petrol are branched hydrocarbons. One example is shown below.
C C
C
H
H
H H
C
H
H
C C
H
H
H
H
H
H
HH
H
H
C
(i) Write the molecular formula for this hydrocarbon.
.............................................................................................................................. [1]
(ii) What is meant by the term hydrocarbon ?
.............................................................................................................................. [1]
(g) State the name of the two products formed when a hydrocarbon burns in excess air.
............................................................. and .............................................................. [2]
[Total: 11]
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5 Ethanol can be made by fermentation.
fermentationmixture
U-shaped tubecontaining water
(a) Apart from yeast, what other substances are present in the reaction mixture? Tick two boxes.
copper sulfate
ethene
sugar
methane
water [2]
(b) What method is used to separate ethanol from the rest of the reaction mixture?
..................................................................................................................................... [1]
(c) Complete the structure of ethanol.
CC
H
H
H
H
H
[1]
(d) Ethanol belongs to the alcohol homologous series. Which one of the following compounds also belongs to the alcohol homologous series? Put a ring around the correct answer.
butene hexane ethanoic acid octanol[1]
(e) Describe one other way, apart from fermentation, by which ethanol can be made on an industrial scale. Include the necessary reaction conditions in your answer.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [3]
[Total: 8]
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6 (a) When hydrated copper(II) sulfate is heated, the following reaction occurs:
CuSO4.5H2O(s) CuSO4(s) + 5H2O(l) hydrated copper(II) sulfate anhydrous copper(II) sulfate
(i) What does the sign mean?
.............................................................................................................................. [1]
(ii) Explain how this reaction is used as a chemical test for water.
....................................................................................................................................
.............................................................................................................................. [2]
(iii) Copper(II) sulfate is a salt. Sodium chloride is also a salt. Solid sodium chloride does not conduct electricity. Suggest two things you could do to make solid sodium chloride conduct electricity.
1. ................................................................................................................................
2. .......................................................................................................................... [2]
(b) Copper ore contains copper, iron and sulfur. Copper is extracted by heating copper ore with sand and oxygen.
(i) In the fi rst stage of this process, the copper ore is heated in a furnace. A liquid mixture containing copper sulfi de and iron sulfi de is formed. The sand reacts
with the impurities to form a slag.
waste gases
oxygen
slag out
mixture out
slag
mixture ofcopper sulfide+ iron sulfide
What information in the diagram above suggests that the slag is less dense than the mixture of copper and iron sulfi des.
.............................................................................................................................. [1]
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(ii) In a later stage, copper sulfi de is reacted with more oxygen.
Cu2S + O2 → 2Cu + SO2
How does this equation show that the sulfur in copper sulfi de gets oxidised?
.............................................................................................................................. [1]
(iii) Copper is purifi ed by electrolysis using copper electrodes.
+ –
A
C
D
B
Which letter, A, B, C or D, in the diagram above represents
the cathode, ...............................................................................................................
the electrolyte? .................................................................................................... [2]
[Total: 9]
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7 The graph below shows how the temperature rises with time when a solid, P, is heated steadily and changes to a liquid and then to a gas.
0 20 40 60
200
180
160
140
120
100
80
60
40
20
0
tem
pera
ture
/ °C
time / seconds
(a) Use the information on the graph to deduce
the melting point of P, .......................................................................................................
the state of P at 160 °C. .............................................................................................. [2]
(b) Explain what happens to the arrangement and motion of the particles when a solid changes to a liquid.
arrangement .....................................................................................................................
motion ......................................................................................................................... [2]
12
0620/23/O/N/13© UCLES 2013
ForExaminer’s
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(c) A student placed a purple crystal in a fl ask of organic solvent. After 10 minutes, the crystal had completely disappeared and a dense purple colour was
observed at the bottom of the fl ask. After 2 hours, the purple colour had spread throughout the solvent.
organicsolvent
crystal at start
after 10 minutes after 2 hours
Use the kinetic particle theory to explain these observations.
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [3]
[Total: 7]
13
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ForExaminer’s
Use
8 (a) State two differences between a mixture and a compound.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
(b) Plant ash is a mixture of large insoluble particles and salts which are soluble in water.
In parts of Africa, salts are traditionally obtained from plant ash. Water is added to the plant ash. The apparatus shown below is then used to remove the insoluble particles.
clay pot
clay bowl
holes inclay bowl
plant ashand water strips of banana leaf
with holes in them
Explain how this apparatus separates the salts from the insoluble particles.
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
14
0620/23/O/N/13© UCLES 2013
ForExaminer’s
Use
(c) The composition and solubility of some salts found in the ash from the papyrus plant are shown in the table below.
salt ion presentin the salt
mass of salt per100 g of ash / g
solubility of saltin g / dm3
magnesium sulfate Mg2+ and SO42– 5 220
potassium carbonate K+ and CO32– 10 1120
potassium chloride K+ and Cl – 18 359
potassium sulfate 4 122
sodium carbonate Na+ and CO32– 12 70
sodium chloride Na+ and Cl – 40 359
(i) Which salt in the table has the lowest solubility in g / dm3?
.............................................................................................................................. [1]
(ii) Which negatively-charged ion is present in the highest amount in the ash?
.............................................................................................................................. [1]
(iii) Write the symbols for the two ions present in potassium sulfate.
.............................................................................................................................. [2]
(d) Sodium chloride reacts with lead(II) nitrate to form sodium nitrate and lead(II) chloride. Complete the symbol equation for this reaction.
.......NaCl + Pb(NO3)2 → 2NaNO3 + PbCl 2[1]
(e) Complete the following sentence about the formation of chloride ions.
Chloride ions are formed when chlorine atoms gain .................................... . [1]
[Total: 10]
15
0620/23/O/N/13
BLANK PAGE
© UCLES 2013
16
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Everyreasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included the publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
0620/23/O/N/13© UCLES 2013
Gro
up
140
Ce
Cer
ium
58
141
PrP
rase
odym
ium
59
144
Nd
Neo
dym
ium
60
PmP
rom
ethi
um61
150
SmS
amar
ium
62
152
EuE
urop
ium
63
157
Gd
Gad
olin
ium
64
159
Tb Terb
ium
65
162
Dy
Dys
pros
ium
66
165
Ho
Hol
miu
m67
167
Er Erb
ium
68
169
Tm Thul
ium
69
173
YbY
tterb
ium
70
175
LuLu
tetiu
m71
232
Th Thor
ium
90
PaP
rota
ctin
ium
91
238 U
Ura
nium
92
Np
Nep
tuni
um93
PuP
luto
nium
94
Am
Am
eric
ium
95
Cm
Cur
ium
96
Bk
Ber
keliu
m97
Cf
Cal
iforn
ium
98
EsE
inst
eini
um99
Fm Ferm
ium
100
Md
Men
dele
vium
101
No
Nob
eliu
m10
2
LrLa
wre
nciu
m10
3
1 HH
ydro
gen
1
7 LiLi
thiu
m3
23 Na
Sod
ium
11
24 Mg
Mag
nesi
um12
40 Ca
Cal
cium
20
45 ScS
cand
ium
21
48 TiTi
tani
um22
51 VVa
nadi
um23
52 Cr
Chr
omiu
m24
55 Mn
Man
gane
se25
56 Fe Iron
26
59 Co
Cob
alt
27
59 Ni
Nic
kel
28
64 Cu
Cop
per
29
65 Zn Zinc
30
70 Ga
Gal
lium
31
27 Al
Alu
min
ium
13
11 B Bor
on5
12 CC
arbo
n6
14 NN
itrog
en7
16 OO
xyge
n8
19 FFl
uorin
e9
28 Si Sili
con
14
31 PP
hosp
horu
s15
32 S Sul
fur
16
35.5 Cl
Chl
orin
e17
40 Ar
Arg
on18
20 Ne
Neo
n10
4 He
Hel
ium
2
73 Ge
Ger
man
ium
32
75 As
Ars
enic
33
79 SeS
elen
ium
34
80 Br
Bro
min
e35
84 Kr
Kry
pton
36
39 KP
otas
sium
19
88 SrS
tront
ium
38
89 YY
ttriu
m39
91 ZrZi
rcon
ium
40
93 Nb
Nio
bium
41
96 Mo
Mol
ybde
num
42
TcTe
chne
tium
43
101
Ru
Rut
heni
um44
103
Rh
Rho
dium
45
106
PdP
alla
dium
46
108
Ag
Silv
er47
112
Cd
Cad
miu
m48
115
In Indi
um49
119
Sn Tin
50
122
SbA
ntim
ony
51
128
TeTe
lluriu
m52
127 I
Iodi
ne53
131
Xe Xen
on54
137
Ba
Bar
ium
56
139
LaLa
ntha
num
57
*
178
Hf
Haf
nium
72
181
TaTa
ntal
um73
184 W
Tung
sten
74
186
Re
Rhe
nium
75
190
Os
Osm
ium
76
192
Ir Iridi
um77
195 Pt
Pla
tinum
78
197
Au
Gol
d79
201
Hg
Mer
cury
80
204 Tl
Thal
lium
81
207
Pb Lead
82
209 Bi
Bis
mut
h83
PoP
olon
ium
84
At
Ast
atin
e85
Rn
Rad
on86
FrFr
anci
um87
227
Ac
Act
iniu
m89
9 Be
Ber
ylliu
m4
III
IIIIV
VV
IV
II0
85 Rb
Rub
idiu
m37
133
Cs
Cae
sium
55
226
Ra
Rad
ium
88
The
volu
me
of o
ne m
ole
of a
ny g
as is
24
dm3
at ro
om te
mpe
ratu
re a
nd p
ress
ure
(r.t.p
.).
a Xb
a =
rela
tive
atom
ic m
ass
X =
atom
ic s
ymbo
l
b =
prot
on (a
tom
ic) n
umbe
r
Key
* 58-
71 L
anth
anoi
d se
ries
90-1
03 A
ctin
oid
serie
s
DAT
A SH
EET
The
Perio
dic
Tabl
e of
the
Elem
ents
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.Write in dark blue or black pen.You may use a pencil for any diagrams, graphs or rough working.Do not use staples, paper clips, highlighters, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.
Answer all questions.Electronic calculators may be used.A copy of the Periodic Table is printed on page 16.You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.
CHEMISTRY 0620/31
Paper 3 (Extended) October/November 2013
1 hour 15 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONSInternational General Certifi cate of Secondary Education
This document consists of 14 printed pages and 2 blank pages.
[Turn overIB13 11_0620_31/3RP R© UCLES 2013
2
0620/31/O/N/13© UCLES 2013
ForExaminer’s
Use
1 For each of the following, name an element which matches the description.
(a) It is used as a fuel in nuclear reactors.
..................................................................................................................................... [1]
(b) It is the only non-metal which is a good conductor of electricity.
..................................................................................................................................... [1]
(c) Inert electrodes are made from this metal.
..................................................................................................................................... [1]
(d) This gaseous element is used to fi ll balloons in preference to hydrogen.
..................................................................................................................................... [1]
(e) An element which can form an ion of the type X3–.
..................................................................................................................................... [1]
(f) It has the same electron distribution as the calcium ion, Ca2+.
..................................................................................................................................... [1]
(g) The element is in Period 5 and Group VI.
..................................................................................................................................... [1]
[Total: 7]
3
0620/31/O/N/13© UCLES 2013 [Turn over
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2 (a) Give three differences in physical properties between the Group I metal, potassium, and the transition element, iron.
1. .......................................................................................................................................
2. .......................................................................................................................................
3. ................................................................................................................................. [3]
(b) The following metals are in order of reactivity.
potassium zinc copper
For those metals which react with water or steam, name the products of the reaction, otherwise write ‘no reaction’.
potassium .........................................................................................................................
...........................................................................................................................................
zinc ...................................................................................................................................
...........................................................................................................................................
copper ...............................................................................................................................
..................................................................................................................................... [5]
[Total: 8]
4
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3 Ammonia is manufactured by the Haber process.
N2(g) + 3H2(g) 2NH3(g)
The forward reaction is exothermic.
(a) Describe how the reactants are obtained.
(i) Nitrogen
....................................................................................................................................
.............................................................................................................................. [2]
(ii) Hydrogen
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [3]
(b) The percentage of ammonia in the equilibrium mixture varies with temperature and pressure.
(i) Which pair of graphs, A, B or C, shows correctly how the percentage of ammonia at equilibrium varies with temperature and pressure?
percentageNH3 atequilibrium
temperature
percentageNH3 atequilibrium
pressure
pair A
percentageNH3 atequilibrium
temperature
percentageNH3 atequilibrium
pressure
pair B
percentageNH3 atequilibrium
temperature
percentageNH3 atequilibrium
pressure
pair C
The pair with both graphs correct is ................................................................. [1]
5
0620/31/O/N/13© UCLES 2013 [Turn over
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Use
(ii) Give a full explanation of why the pair of graphs you have chosen in (i) is correct.
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [6]
(iii) Catalysts do not alter the position of equilibrium. Explain why a catalyst is used in this process.
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [2]
[Total: 14]
6
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Use
4 20.0 g of small lumps of calcium carbonate and 40 cm3 of hydrochloric acid, concentration 2.0 mol / dm3, were placed in a fl ask on a top pan balance. The mass of the fl ask and contents was recorded every minute.
cotton wool to preventdrops of acid spray escaping
flask
40 cm3 of hydrochloric acid, 2.0 mol / dm3
20.0 g of small lumps ofcalcium carbonate
balance
The mass of carbon dioxide given off was plotted against time.
00 time
mass ofcarbon dioxide
CaCO3(s) + 2HCl (aq) CaCl 2(aq) + H2O(l) + CO2(g)
In all the experiments mentioned in this question, the calcium carbonate was in excess.
(a) (i) Explain how you could determine the mass of carbon dioxide given off in the fi rst fi ve minutes.
.............................................................................................................................. [1]
(ii) Label the graph F where the reaction rate is the fastest, S where it is slowing down and 0 where the rate is zero. [2]
(iii) Explain how the shape of the graph shows where the rate is fastest, where it is slowing down and where the rate is zero.
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [2]
(b) Sketch on the same graph, the line which would have been obtained if 20.0 g of small lumps of calcium carbonate and 80 cm3 of hydrochloric acid, concentration 1.0 mol / dm3, had been used. [2]
7
0620/31/O/N/13© UCLES 2013 [Turn over
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(c) Explain in terms of collisions between reacting particles each of the following.
(i) The reaction rate would be slower if 20.0 g of larger lumps of calcium carbonate and 40 cm3 of hydrochloric acid, concentration 2.0 mol / dm3, were used.
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [2]
(ii) The reaction rate would be faster if the experiment was carried out at a higher temperature.
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [2]
(d) Calculate the maximum mass of carbon dioxide given off when 20.0 g of small lumps of calcium carbonate react with 40 cm3 of hydrochloric acid, concentration 2.0 mol / dm3.
CaCO3(s) + 2HCl (aq) CaCl 2(aq) + H2O(l) + CO2(g)
number of moles of HCl used =
mass of carbon dioxide = ................. g [4]
[Total: 15]
8
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Use
5 The alkenes are unsaturated hydrocarbons. They form a homologous series, the members of which have the same chemical properties.
They undergo addition reactions and are easily oxidised.
(a) The following hydrocarbons are isomers.
CH3
CH3
CH2CH CH CH3 CH2CH2CH2 CH
(i) Explain why these two hydrocarbons are isomers.
....................................................................................................................................
.............................................................................................................................. [2]
(ii) Give the structural formula of another hydrocarbon which is isomeric with the above.
[1]
(b) Give the structural formula and name of each of the products of the following addition reactions.
(i) ethene and bromine
structural formula of product
name of product ................................................................................................... [2]
(ii) propene and hydrogen
structural formula of product
name of product ................................................................................................... [2]
(iii) but-1-ene and water
structural formula of product
name of product ................................................................................................... [2]
9
0620/31/O/N/13© UCLES 2013 [Turn over
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(c) Alkenes can be oxidised to carboxylic acids.
(i) For example, propene, CH3 – CH = CH2, would produce ethanoic acid, CH3 – COOH, and methanoic acid, H – COOH. Deduce the formulae of the alkenes which would form the following carboxylic acids when oxidised.
ethanoic acid and propanoic acid
only ethanoic acid
[2]
(ii) Describe the colour change you would observe when an alkene is oxidised with acidifi ed potassium manganate(VII).
.............................................................................................................................. [2]
(d) Alkenes polymerise to form addition polymers. Draw the structural formula of poly(cyanoethene), include at least two monomer units.
The structural formula of the monomer, cyanoethene, is given below.
C C
H
CN
H
H
[3]
[Total: 16]
10
0620/31/O/N/13© UCLES 2013
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Use
6 Lead is an excellent roofi ng material. It is malleable and resistant to corrosion. Lead rapidly becomes coated with basic lead carbonate which protects it from further corrosion.
(a) Lead has a typical metallic structure which is a lattice of lead ions surrounded by a ‘sea’ of mobile electrons. This structure is held together by attractive forces called a metallic bond.
(i) Explain why there are attractive forces in a metallic structure.
....................................................................................................................................
.............................................................................................................................. [2]
(ii) Explain why a metal, such as lead, is malleable.
....................................................................................................................................
.............................................................................................................................. [2]
(b) Basic lead(II) carbonate is heated in the apparatus shown below. Water and carbon dioxide are produced.
soda lime,carbon dioxidereacts here
basic leadcarbonate
heat
U-tube filledwith silica gel
to absorb water
(i) Silica gel absorbs water. Silica gel often contains anhydrous cobalt(II) chloride. When this absorbs water it changes from blue to pink.
Suggest a reason.
.............................................................................................................................. [1]
(ii) Soda lime is a mixture of sodium hydroxide and calcium oxide. Why do these two substances react with carbon dioxide?
....................................................................................................................................
.............................................................................................................................. [2]
(iii) Name two substances formed when soda lime reacts with carbon dioxide.
.............................................................................................................................. [2]
11
0620/31/O/N/13© UCLES 2013 [Turn over
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(c) Basic lead(II) carbonate has a formula of the type xPbCO3.yPb(OH)2 where x and y are whole numbers.
Determine x and y from the following information.
PbCO3 PbO + CO2
Pb(OH)2 PbO + H2O
When heated, the basic lead(II) carbonate gave 2.112 g of carbon dioxide and 0.432 g of water.
Mass of one mole of CO2 = 44 g Mass of one mole of H2O = 18 g
Number of moles of CO2 formed = ..................... [1]
Number of moles of H2O formed = ..................... [1]
x = ..................... and y = .....................
Formula of basic lead(II) carbonate is ........................................................................ [1]
[Total: 12]
12
0620/31/O/N/13© UCLES 2013
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Use
7 (a) The following are two examples of substitution reactions. Only the reaction involving chlorine is a photochemical reaction.
CH4 + Cl 2 CH3Cl + HCl
CH4 + Br2 CH3Br + HBr
(i) Explain the phrase substitution reaction.
....................................................................................................................................
.............................................................................................................................. [1]
(ii) How do photochemical reactions differ from other reactions?
....................................................................................................................................
.............................................................................................................................. [1]
(b) Bond forming is exothermic, bond breaking is endothermic. Explain the difference between an exothermic reaction and an endothermic reaction.
...........................................................................................................................................
..................................................................................................................................... [2]
13
0620/31/O/N/13© UCLES 2013 [Turn over
ForExaminer’s
Use
(c) Use the bond energies to show that the following reaction is exothermic. Bond energy is the amount of energy (kJ / mol) which must be supplied to break one mole
of the bond.
H C
H
H
H H C
H
H
Cl Cl Cl H Cl+ +→
Bond energies in kJ / mol
Cl –Cl +242 C–Cl +338 C–H +412 H–Cl +431
bonds broken energy in kJ / mol
...................... .............................
...................... .............................
total energy = .............................
bonds formed energy in kJ / mol
...................... .............................
...................... .............................
total energy = .............................
...........................................................................................................................................
..................................................................................................................................... [4]
[Total: 8]
14
0620/31/O/N/13
BLANK PAGE
© UCLES 2013
15
0620/31/O/N/13
BLANK PAGE
© UCLES 2013
16
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Everyreasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included the publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
0620/31/O/N/13© UCLES 2013
Gro
up
140
Ce
Cer
ium
58
141
PrP
rase
odym
ium
59
144
Nd
Neo
dym
ium
60
PmP
rom
ethi
um61
150
SmS
amar
ium
62
152
EuE
urop
ium
63
157
Gd
Gad
olin
ium
64
159
Tb Terb
ium
65
162
Dy
Dys
pros
ium
66
165
Ho
Hol
miu
m67
167
Er Erb
ium
68
169
Tm Thul
ium
69
173
YbY
tterb
ium
70
175
LuLu
tetiu
m71
232
Th Thor
ium
90
PaP
rota
ctin
ium
91
238 U
Ura
nium
92
Np
Nep
tuni
um93
PuP
luto
nium
94
Am
Am
eric
ium
95
Cm
Cur
ium
96
Bk
Ber
keliu
m97
Cf
Cal
iforn
ium
98
EsE
inst
eini
um99
Fm Ferm
ium
100
Md
Men
dele
vium
101
No
Nob
eliu
m10
2
LrLa
wre
nciu
m10
3
1 HH
ydro
gen
1
7 LiLi
thiu
m3
23 Na
Sod
ium
11
24 Mg
Mag
nesi
um12
40 Ca
Cal
cium
20
45 ScS
cand
ium
21
48 TiTi
tani
um22
51 VVa
nadi
um23
52 Cr
Chr
omiu
m24
55 Mn
Man
gane
se25
56 Fe Iron
26
59 Co
Cob
alt
27
59 Ni
Nic
kel
28
64 Cu
Cop
per
29
65 Zn Zinc
30
70 Ga
Gal
lium
31
27 Al
Alu
min
ium
13
11 B Bor
on5
12 CC
arbo
n6
14 NN
itrog
en7
16 OO
xyge
n8
19 FFl
uorin
e9
28 Si Sili
con
14
31 PP
hosp
horu
s15
32 S Sul
fur
16
35.5 Cl
Chl
orin
e17
40 Ar
Arg
on18
20 Ne
Neo
n10
4 He
Hel
ium
2
73 Ge
Ger
man
ium
32
75 As
Ars
enic
33
79 SeS
elen
ium
34
80 Br
Bro
min
e35
84 Kr
Kry
pton
36
39 KP
otas
sium
19
88 SrS
tront
ium
38
89 YY
ttriu
m39
91 ZrZi
rcon
ium
40
93 Nb
Nio
bium
41
96 Mo
Mol
ybde
num
42
TcTe
chne
tium
43
101
Ru
Rut
heni
um44
103
Rh
Rho
dium
45
106
PdP
alla
dium
46
108
Ag
Silv
er47
112
Cd
Cad
miu
m48
115
In Indi
um49
119
Sn Tin
50
122
SbA
ntim
ony
51
128
TeTe
lluriu
m52
127 I
Iodi
ne53
131
Xe Xen
on54
137
Ba
Bar
ium
56
139
LaLa
ntha
num
57
*
178
Hf
Haf
nium
72
181
TaTa
ntal
um73
184 W
Tung
sten
74
186
Re
Rhe
nium
75
190
Os
Osm
ium
76
192
Ir Iridi
um77
195 Pt
Pla
tinum
78
197
Au
Gol
d79
201
Hg
Mer
cury
80
204 Tl
Thal
lium
81
207
Pb Lead
82
209 Bi
Bis
mut
h83
PoP
olon
ium
84
At
Ast
atin
e85
Rn
Rad
on86
FrFr
anci
um87
227
Ac
Act
iniu
m89
9 Be
Ber
ylliu
m4
III
IIIIV
VV
IV
II0
85 Rb
Rub
idiu
m37
133
Cs
Cae
sium
55
226
Ra
Rad
ium
88
The
volu
me
of o
ne m
ole
of a
ny g
as is
24
dm3
at ro
om te
mpe
ratu
re a
nd p
ress
ure
(r.t.p
.).
a Xb
a =
rela
tive
atom
ic m
ass
X =
atom
ic s
ymbo
l
b =
prot
on (a
tom
ic) n
umbe
r
Key
* 58-
71 L
anth
anoi
d se
ries
90-1
03 A
ctin
oid
serie
s
DAT
A SH
EET
The
Perio
dic
Tabl
e of
the
Elem
ents
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.Write in dark blue or black pen.You may use a pencil for any diagrams, graphs or rough working.Do not use staples, paper clips, highlighters, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.
Answer all questions.Electronic calculators may be used.A copy of the Periodic Table is printed on page 16.You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.
CHEMISTRY 0620/32
Paper 3 (Extended) October/November 2013
1 hour 15 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONSInternational General Certifi cate of Secondary Education
This document consists of 14 printed pages and 2 blank pages.
[Turn overIB13 11_0620_32/2RP© UCLES 2013
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1 The table gives the melting points, the boiling points and the electrical properties of six substances A to F.
substance melting point/ °C
boiling point/ °C
electrical conductivityas a solid
electrical conductivityas a liquid
A –210 –196 does not conduct does not conduct
B 777 1627 does not conduct good conductor
C 962 2212 good conductor good conductor
D –94 63 does not conduct does not conduct
E 1410 2355 does not conduct does not conduct
F 1064 2807 good conductor good conductor
(a) Which two substances could be metals? ................................................................... [1]
(b) Which substance could be nitrogen? .......................................................................... [1]
(c) Which substance is an ionic solid? ............................................................................. [1]
(d) Which substance is a liquid at room temperature? ..................................................... [1]
(e) Which substance has a giant covalent structure similar to that of diamond? .............. [1]
(f) Which two substances could exist as simple covalent molecules? ........................... [1]
[Total: 6]
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2 The halogens are a collection of diatomic non-metals in Group VII.
(a) (i) Defi ne the term diatomic.
.............................................................................................................................. [1]
(ii) What do the electron distributions of the halogens have in common?
.............................................................................................................................. [1]
(iii) How do their electron distributions differ?
.............................................................................................................................. [1]
(iv) Complete the table.
halogen solid, liquid or gasat room temperature colour
chlorine ......................................... .........................................
bromine ......................................... .........................................
iodine ......................................... .........................................[2]
(b) The halogens react with other non-metals to form covalent compounds. Draw a diagram which shows the arrangement of the valency electrons in one molecule
of the covalent compound arsenic trifl uoride. The electron distribution of an arsenic atom is 2 + 8 + 18 + 5.
Use x to represent an electron from an arsenic atom. Use o to represent an electron from a fl uorine atom.
[3]
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(c) Photochromic glass is used in sunglasses. In bright light, the glass darkens reducing the amount of light reaching the eye. When the light is less bright, the glass becomes colourless increasing the amount of light reaching the eye.
Photochromic glass contains very small amounts of the halides silver(I) chloride and copper(I) chloride.
The reaction between these two chlorides is photochemical.
AgCl + CuCl Ag + CuCl 2 colourless colourless black colourless
How does photochromic glass work?
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [3]
[Total: 11]
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3 (a) Nitric acid is now made by the oxidation of ammonia. It used to be made from air and water. This process used very large amounts of electricity.
Air was blown through an electric arc and heated to 3000 °C.
N2(g) + O2(g) 2NO(g) equilibrium 1 nitric oxide
The equilibrium mixture leaving the arc contained 5 % of nitric oxide. This mixture was cooled rapidly. At lower temperatures, nitric oxide will react with oxygen to form nitrogen dioxide.
2NO(g) + O2(g) 2NO2 equilibrium 2
Nitrogen dioxide reacts with oxygen and water to form nitric acid.
(i) Suggest a reason why the yield of nitric oxide in equilibrium 1 increases with temperature.
.............................................................................................................................. [1]
(ii) What effect, if any, would increasing the pressure have on the percentage of nitric oxide in equilibrium 1? Explain your answer.
....................................................................................................................................
.............................................................................................................................. [2]
(iii) Deduce why equilibrium 2 is only carried out at lower temperatures.
....................................................................................................................................
.............................................................................................................................. [2]
(iv) Complete the equation for the reaction between nitrogen dioxide, water and oxygen to form nitric acid.
........NO2 + O2 + ............ → ............HNO3 [2]
(v) Ammonia is more expensive than water and air. Suggest a reason why theammonia-based process is preferred to the electric arc process.
.............................................................................................................................. [1]
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(b) (i) Nitric acid is used to make the fertiliser ammonium nitrate, NH4NO3. What advantage has this fertiliser over another common fertiliser, ammonium sulfate,
(NH4)2SO4?
.............................................................................................................................. [1]
(ii) Plants need nitrogen to make chlorophyll. Explain why chlorophyll is essential for plant growth.
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [4]
[Total: 13]
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4 For centuries, iron has been extracted from its ore in the blast furnace. The world production of pig iron is measured in hundreds of million tonnes annually.
(a) The following raw materials are supplied to a modern blast furnace.
iron ore which is hematite, Fe2O3
limestone which is calcium carbonate carbon in the form of coke air
Describe the essential reactions in the blast furnace. Each of the four raw materials must be mentioned at least once. Give the equation for the reduction of hematite.
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [6]
(b) Each year, blast furnaces discharge millions of tonnes of carbon dioxide into the atmosphere. This will increase the percentage of atmospheric carbon dioxide.
(i) Explain why this increased percentage of carbon dioxide may cause problems in the future.
....................................................................................................................................
.............................................................................................................................. [2]
(ii) Until the early eighteenth century, charcoal, not coke, was used in the blast furnace. Charcoal is made from wood but coke is made from coal. Explain why the use of charcoal would have a smaller effect on the level of atmospheric carbon dioxide.
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [2]
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(iii) A method being developed to produce iron with lower emissions of carbon dioxide is by electrolysis. Hematite, Fe2O3, is dissolved in molten lithium carbonate and electrolysed. The ore is spilt into its constituent elements.
Write an equation for the reaction at the negative electrode (cathode).
....................................................................................................................................
Complete the equation for the reaction at the positive electrode (anode).
........O2– → ............... + ............... [3]
[Total: 13]
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5 Silver(I) chromate(VI) is an insoluble salt. It is prepared by precipitation. 20 cm3 of aqueous silver(I) nitrate, concentration 0.2 mol / dm3, was mixed with 20 cm3 of
aqueous potassium chromate(VI), concentration 0.1 mol / dm3. After stirring, the mixture was fi ltered. The precipitate was washed several times with distilled water. The precipitate was then left in a warm oven for several hours.
2AgNO3(aq) + K2CrO4(aq) → Ag2CrO4(s) + 2KNO3(aq)
(a) What diffi culty arises if the name of a compound of a transition element does not include its oxidation state, for example iron oxide?
...........................................................................................................................................
..................................................................................................................................... [2]
(b) These questions refer to the preparation of the salt.
(i) Why is it necessary to fi lter the mixture after mixing and stirring?
.............................................................................................................................. [1]
(ii) What is the purpose of washing the precipitate?
.............................................................................................................................. [1]
(iii) Why leave the precipitate in a warm oven?
.............................................................................................................................. [1]
(c) (i) Explain why the concentrations of silver(I) nitrate and potassium chromate(VI) are different.
.............................................................................................................................. [1]
(ii) What mass of silver(I) nitrate is needed to prepare 100 cm3 of silver(I) nitrate solution, concentration 0.2 mol / dm3?
The mass of one mole of AgNO3 is 170 g.
....................................................................................................................................
.............................................................................................................................. [2]
(iii) What is the maximum mass of silver(I) chromate(VI) which could be obtained from 20 cm3 of aqueous silver(I) nitrate, concentration 0.2 mol / dm3?
number of moles of AgNO3 used = ..................... [1]
number of moles of Ag2CrO4 formed = ..................... [1]
mass of one mole of Ag2CrO4 = 332 g
mass of Ag2CrO4 formed = ..................... g [1]
[Total: 11]
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6 The following reactivity series shows both familiar and unfamiliar elements in order of decreasing reactivity. Each element is represented by a redox equation.
Rb Rb+ + e–
Mg Mg2+ + 2e–
Mn Mn2+ + 2e–
Zn Zn2+ + 2e–
H2 2H+ + 2e–
Cu Cu2+ + 2e–
Hg Hg2+ + 2e–
Two of the uses of the series are to predict the thermal stability of compounds of the metals and to explain their redox reactions.
(a) Most metal hydroxides decompose when heated.
(i) Complete the equation for the thermal decomposition of copper(II) hydroxide.
Cu(OH)2 → ............... + ............... [1]
(ii) Choose a metal from the above series whose hydroxide does not decompose when heated.
.............................................................................................................................. [1]
(b) (i) Defi ne in terms of electron transfer the term oxidation.
.............................................................................................................................. [1]
(ii) Explain why the positive ions in the above equations are oxidising agents.
....................................................................................................................................
.............................................................................................................................. [1]
(c) (i) Which metals in the series above do not react with dilute acids to form hydrogen?
.............................................................................................................................. [1]
(ii) Describe an experiment which would confi rm the prediction made in (c)(i).
....................................................................................................................................
.............................................................................................................................. [1]
(d) (i) Which metal in the series above can form a negative ion which gives a pink / purple solution in water?
.............................................................................................................................. [1]
(ii) Describe what you would observe when zinc, a reducing agent, is added to this pink / purple solution.
.............................................................................................................................. [1]
[Total: 8]
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7 Plants can make complex molecules from simple starting materials, such as water, carbon dioxide and nitrates. Substances produced by plants include sugars, more complex carbohydrates, esters, proteins, vegetable oils and fats.
(a) (i) Describe how you could decide from its molecular formula whether a compound is a carbohydrate.
....................................................................................................................................
.............................................................................................................................. [2]
(ii) Plants can change the sugar, glucose, into starch which is a more complex carbohydrate. What type of reaction is this?
.............................................................................................................................. [2]
(b) The fermentation of glucose can be carried out in the apparatus shown below. After a few days the reaction stops. A 12% aqueous solution of ethanol has been produced.
water allows carbondioxide to escape butprevents air from entering
aqueous glucoseand yeast
(i) The enzyme, zymase, catalyses the anaerobic respiration of the yeast. Explain the term respiration.
....................................................................................................................................
.............................................................................................................................. [2]
(ii) Complete the equation.
C6H12O6 → ......................... + ................................... [2] glucose ethanol carbon dioxide
(iii) Why must air be kept out of the fl ask?
.............................................................................................................................. [1]
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(c) The ester methyl butanoate is found in apples. It can be made from butanoic acid and methanol. Their structural formulae are given below.
C
H
H
C
O
O H
C
H
H
C
H
H
H HOC
H
H
H
butanoic acid methanol
Use the information given above to deduce the structural formula of methyl butanoate showing all the bonds.
[2]
(d) The equation represents the hydrolysis of a naturally occurring ester.
C17H35 CO2 CH2
C17H35 CO2 3C17H35COONa CHOHCH 3NaOH+ +→
C17H35 CO2 CH2
CH2OH
CH2OH
(i) Which substance in the equation is an alcohol? Put a ring around this substance in the equation above. [1]
(ii) Is the alkyl group, C17H35, in this ester saturated or unsaturated? Give a reason for your choice.
.............................................................................................................................. [1]
(iii) What type of compound is represented by the formula C17H35COONa? What is the major use for compounds of this type?
type of compound ......................................................................................................
use ....................................................................................................................... [2]
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(e) Proteins are natural macromolecules. Draw the structural formula of a typical protein. Include three monomer units. You may represent amino acids by formulae of the type drawn below.
H2N COOH H2N COOH
[3]
[Total: 18]
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16
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University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
0620/32/O/N/13© UCLES 2013
Gro
up
140
Ce
Cer
ium
58
141
PrP
rase
odym
ium
59
144
Nd
Neo
dym
ium
60
PmP
rom
ethi
um61
150
SmS
amar
ium
62
152
EuE
urop
ium
63
157
Gd
Gad
olin
ium
64
159
Tb Terb
ium
65
162
Dy
Dys
pros
ium
66
165
Ho
Hol
miu
m67
167
Er Erb
ium
68
169
Tm Thul
ium
69
173
YbY
tterb
ium
70
175
LuLu
tetiu
m71
232
Th Thor
ium
90
PaP
rota
ctin
ium
91
238 U
Ura
nium
92
Np
Nep
tuni
um93
PuP
luto
nium
94
Am
Am
eric
ium
95
Cm
Cur
ium
96
Bk
Ber
keliu
m97
Cf
Cal
iforn
ium
98
EsE
inst
eini
um99
Fm Ferm
ium
100
Md
Men
dele
vium
101
No
Nob
eliu
m10
2
LrLa
wre
nciu
m10
3
1 HH
ydro
gen
1
7 LiLi
thiu
m3
23 Na
Sod
ium
11
24 Mg
Mag
nesi
um12
40 Ca
Cal
cium
20
45 ScS
cand
ium
21
48 TiTi
tani
um22
51 VVa
nadi
um23
52 Cr
Chr
omiu
m24
55 Mn
Man
gane
se25
56 Fe Iron
26
59 Co
Cob
alt
27
59 Ni
Nic
kel
28
64 Cu
Cop
per
29
65 Zn Zinc
30
70 Ga
Gal
lium
31
27 Al
Alu
min
ium
13
11 B Bor
on5
12 CC
arbo
n6
14 NN
itrog
en7
16 OO
xyge
n8
19 FFl
uorin
e9
28 Si Sili
con
14
31 PP
hosp
horu
s15
32 S Sul
fur
16
35.5 Cl
Chl
orin
e17
40 Ar
Arg
on18
20 Ne
Neo
n10
4 He
Hel
ium
2
73 Ge
Ger
man
ium
32
75 As
Ars
enic
33
79 SeS
elen
ium
34
80 Br
Bro
min
e35
84 Kr
Kry
pton
36
39 KP
otas
sium
19
88 SrS
tront
ium
38
89 YY
ttriu
m39
91 ZrZi
rcon
ium
40
93 Nb
Nio
bium
41
96 Mo
Mol
ybde
num
42
TcTe
chne
tium
43
101
Ru
Rut
heni
um44
103
Rh
Rho
dium
45
106
PdP
alla
dium
46
108
Ag
Silv
er47
112
Cd
Cad
miu
m48
115
In Indi
um49
119
Sn Tin
50
122
SbA
ntim
ony
51
128
TeTe
lluriu
m52
127 I
Iodi
ne53
131
Xe Xen
on54
137
Ba
Bar
ium
56
139
LaLa
ntha
num
57
*
178
Hf
Haf
nium
72
181
TaTa
ntal
um73
184 W
Tung
sten
74
186
Re
Rhe
nium
75
190
Os
Osm
ium
76
192
Ir Iridi
um77
195 Pt
Pla
tinum
78
197
Au
Gol
d79
201
Hg
Mer
cury
80
204 Tl
Thal
lium
81
207
Pb Lead
82
209 Bi
Bis
mut
h83
PoP
olon
ium
84
At
Ast
atin
e85
Rn
Rad
on86
FrFr
anci
um87
227
Ac
Act
iniu
m89
9 Be
Ber
ylliu
m4
III
IIIIV
VV
IV
II0
85 Rb
Rub
idiu
m37
133
Cs
Cae
sium
55
226
Ra
Rad
ium
88
The
volu
me
of o
ne m
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of a
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as is
24
dm3
at ro
om te
mpe
ratu
re a
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ress
ure
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.).
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a =
rela
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ass
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atom
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ymbo
l
b =
prot
on (a
tom
ic) n
umbe
r
Key
* 58-
71 L
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90-1
03 A
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DAT
A SH
EET
The
Perio
dic
Tabl
e of
the
Elem
ents
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.Write in dark blue or black pen.You may use a pencil for any diagrams, graphs or rough working.Do not use staples, paper clips, highlighters, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.
Answer all questions.Electronic calculators may be used.A copy of the Periodic Table is printed on page 12.You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.
CHEMISTRY 0620/33
Paper 3 (Extended) October/November 2013
1 hour 15 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONSInternational General Certifi cate of Secondary Education
This document consists of 12 printed pages.
[Turn overIB13 11_0620_33/3RP© UCLES 2013
*1277729958*
2
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1 Zirconium (Zr) is a metal in Period 5. Its main oxidation state is +4.
(a) The following are all zirconium atoms: 90Zr40 , 91Zr40 and 92Zr40 .
In terms of numbers of electrons, neutrons and protons, how are these three atoms the same and how are they different?
They are the same because .............................................................................................
...........................................................................................................................................
They are different because ...............................................................................................
..................................................................................................................................... [3]
(b) Containers for fuel rods in nuclear reactors are made of zirconium. Nuclear reactors are used to produce energy and to make radioactive isotopes.
(i) Which isotope of a different element is used as a fuel in nuclear reactors?
.............................................................................................................................. [1]
(ii) State one medical and one industrial use of radioactive isotopes.
....................................................................................................................................
.............................................................................................................................. [2]
(iii) Above 900 °C, zirconium reacts with water to form zirconium(IV) oxide, ZrO2, and hydrogen. Write an equation for this reaction.
.............................................................................................................................. [2]
(iv) In a nuclear accident, water may come in contact with very hot zirconium. Explain why the presence of hydrogen inside the reactor greatly increases the
danger of the accident.
.............................................................................................................................. [1]
(c) It is possible to determine whether zirconium(IV) oxide is acidic, neutral, basic or amphoteric using an acid and an alkali. Complete the table of possible results. If the oxide is predicted to react write ‘R’, if it is predicted not to react write ‘NR’.
if the oxide is predicted result withhydrochloric acid
predicted result with aqueoussodium hydroxide
acidic
neutral
basic
amphoteric
[4]
[Total: 13]
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2 (a) The diagram shows the lattice of a typical ionic compound.
–
+
–
+
–
–
+
– +
+
–
+
– + – +
+
–
–
– +
+
+
–
(i) Explain the term ionic lattice.
....................................................................................................................................
.............................................................................................................................. [2]
(ii) In this lattice, the ratio of positive ions to negative ions is 1:1. In the lattice of a different ionic compound, the ratio of positive ions to negative ions
is 1:2. Suggest why this ratio varies in different ionic compounds.
.............................................................................................................................. [1]
(iii) Give three physical properties of ionic compounds.
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [3]
(b) Strontium oxide is an ionic compound. Draw a diagram which shows its formula, the charges on the ions and the arrangement of the valency electrons around the negative ion.
The electron distribution of a strontium atom is 2 + 8 + 18 + 8 + 2.
Use o to represent an electron from a strontium atom. Use x to represent an electron from an oxygen atom.
[3]
[Total: 9]
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3 The main uses of zinc are preventing steel from rusting and making alloys.
(a) The main ore of zinc is zinc blende. Zinc blende consists mainly of zinc sulfi de, ZnS. There are two major methods of extracting zinc from its ore. They are the direct reduction of zinc oxide to zinc and by electrolysis. In both methods, zinc oxide is made from the zinc sulfi de in the ore.
(i) How is zinc oxide made from zinc sulfi de?
....................................................................................................................................
.............................................................................................................................. [1]
(ii) Write an equation for the reaction used to reduce zinc oxide to zinc.
.............................................................................................................................. [1]
(b) In the electrolytic method, zinc oxide reacts with sulfuric acid to form impure aqueous zinc sulfate. This solution contains Ni2+, Co2+ and Cu2+ ions as impurities.
(i) Write the equation for the reaction between zinc oxide and sulfuric acid.
.............................................................................................................................. [1]
(ii) Nickel, cobalt and copper are all less reactive than zinc. Explain why the addition of zinc powder removes these ions from the solution.
....................................................................................................................................
.............................................................................................................................. [2]
(c) The solution of zinc sulfate is electrolysed using inert electrodes. This electrolysis is similar to that of copper(II) sulfate with inert electrodes.
(i) Write the equation for the reaction at the negative electrode (cathode).
.............................................................................................................................. [1]
(ii) Complete the equation for the reaction at the positive electrode (anode).
.........OH– → 2H2O + ......... + .........e– [2]
(iii) The electrolyte changes from zinc sulfate to
.............................................................................................................................. [1]
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(d) (i) Brass is an alloy of copper and zinc. Suggest two reasons why brass is often used in preference to copper.
....................................................................................................................................
.............................................................................................................................. [2]
(ii) Sacrifi cial protection is a method of rust prevention. Explain in terms of electron transfer why steel, which is in electrical contact with zinc, does not rust.
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [4]
[Total: 15]
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4 Sulfuric acid is a strong acid. Hexanesulfonic acid is also a strong acid. It has similar properties to sulfuric acid.
(a) Sulfonic acids are made from alkanes and oleum, H2S2O7.
C6H14 + H2S2O7 → C6H13SO3H + H2SO4
(i) Describe how oleum is made from sulfur by the Contact process. Give equations and reaction conditions.
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [6]
(ii) How is concentrated sulfuric acid made from oleum?
.............................................................................................................................. [1]
(b) The formula of the hexanesulfonate ion is C6H13SO3–.
The formula of the barium ion is Ba2+. What is the formula of barium hexanesulfonate?
..................................................................................................................................... [1]
(c) Complete the following equations.
(i) magnesium + hexanesulfonic → ............................. + ......................... acid ............................. [1]
(ii) calcium + hexanesulfonic → ............................. + ......................... oxide acid ............................. [1]
(iii) .....C6H13SO3H + Na2CO3 → ............................. + ............ + ............ [2]
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(d) (i) Sulfuric acid is a strong acid. You are given aqueous sulfuric acid, concentration 0.1 mol / dm3, and aqueous
hexanesulfonic acid, concentration 0.2 mol / dm3. Describe how you could show that hexanesulfonic acid is also a strong acid.
....................................................................................................................................
.............................................................................................................................. [2]
(ii) Deduce why, for a fair comparison, the two acid solutions must have different concentrations.
....................................................................................................................................
.............................................................................................................................. [1]
(iii) Explain the terms strong acid and weak acid.
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [2]
[Total: 17]
8
0620/33/O/N/13© UCLES 2013
ForExaminer’s
Use
5 Domestic rubbish is disposed of in landfi ll sites. Rubbish could include the following items.
item of rubbish approximate time foritem to break down
newspaper one month
cotton rag six months
woollen glove one year
aluminium container up to 500 years
styrofoam cup 1000 years
(a) Explain why aluminium, a reactive metal, takes so long to corrode.
..................................................................................................................................... [1]
(b) Both paper and cotton are complex carbohydrates. They can be hydrolysed to simple sugars such as glucose.
The formula of glucose can be represented as:
HO OH
Draw the structural formula of a complex carbohydrate, such as cotton. Include at least two glucose units.
[2]
9
0620/33/O/N/13© UCLES 2013 [Turn over
ForExaminer’s
Use
(c) Wool is a protein. It can be hydrolysed to a mixture of monomers by enzymes.
(i) What are enzymes?
....................................................................................................................................
.............................................................................................................................. [2]
(ii) Name another substance which can hydrolyse proteins.
.............................................................................................................................. [1]
(iii) What type of compound are the monomers formed by the hydrolysis of proteins?
.............................................................................................................................. [1]
(iv) Which technique could be used to identify the individual monomers in the mixture?
.............................................................................................................................. [1]
(v) Proteins contain the amide linkage. Name a synthetic macromolecule which contains the same linkage.
.............................................................................................................................. [1]
(d) (i) What is the scientifi c term used to describe polymers which do not break down in landfi ll sites?
.............................................................................................................................. [1]
(ii) Styrofoam is poly(phenylethene). It is an addition polymer. Its structural formula is given below. Deduce the structural formula of the monomer, phenylethene.
n
CH2 CH
C6H5
[1]
[Total: 11]
10
0620/33/O/N/13© UCLES 2013
ForExaminer’s
Use
6 The alcohols form a homologous series. The fi rst fi ve members are given in the table below.
(a)
alcohol formula heat of combustionin kJ / mol
methanol CH3OH 730
ethanol CH3–CH2–OH 1380
propan-1-ol
butan-1-ol CH3–CH2–CH2–CH2–OH 2680
pentan-1-ol CH3–CH2–CH2–CH2–CH2–OH 3350
(i) Complete the table. [2]
(ii) Complete the equation for the combustion of pentan-1-ol in excess oxygen.
C5H11OH + .......O2 → ..................... + ..................... [1]
(b) State three characteristics of a homologous series other than the variation of physical properties down the series.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [3]
(c) The following alcohols are isomers.
CH3–CH2–CH2–CH2–OH and (CH3)2CH–CH2–OH
(i) Explain why they are isomers.
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [2]
(ii) Draw the structural formula of another isomer of the above alcohols.
[1]
11
0620/33/O/N/13© UCLES 2013 [Turn over
ForExaminer’s
Use
(d) Alcohols can be made by fermentation and from petroleum.
(i) Ethanol is made from sugars by fermentation.
C6H12O6 → 2C2H5OH + 2CO2
The mass of one mole of glucose, C6H12O6, is 180 g. Calculate the maximum mass of ethanol which could be obtained from 72 g of
glucose.
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [3]
(ii) Describe how ethanol is made from petroleum.
petroleum (alkanes) → ethene → ethanol
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [3]
[Total: 15]
12
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Everyreasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included the publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
0620/33/O/N/13© UCLES 2013
Gro
up
140
Ce
Cer
ium
58
141
PrP
rase
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59
144
Nd
Neo
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60
PmP
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150
SmS
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62
152
EuE
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63
157
Gd
Gad
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64
159
Tb Terb
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65
162
Dy
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pros
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66
165
Ho
Hol
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167
Er Erb
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68
169
Tm Thul
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173
YbY
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70
175
LuLu
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232
Th Thor
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90
PaP
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91
238 U
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Np
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PuP
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Am
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100
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Men
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7 LiLi
thiu
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23 Na
Sod
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11
24 Mg
Mag
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40 Ca
Cal
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20
45 ScS
cand
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21
48 TiTi
tani
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51 VVa
nadi
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52 Cr
Chr
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55 Mn
Man
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56 Fe Iron
26
59 Co
Cob
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27
59 Ni
Nic
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28
64 Cu
Cop
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29
65 Zn Zinc
30
70 Ga
Gal
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27 Al
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11 B Bor
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12 CC
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14 NN
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16 OO
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19 FFl
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40 Ar
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75 As
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80 Br
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84 Kr
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36
39 KP
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19
88 SrS
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89 YY
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91 ZrZi
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93 Nb
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Mol
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101
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Rut
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Rh
Rho
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106
PdP
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46
108
Ag
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112
Cd
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115
In Indi
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119
Sn Tin
50
122
SbA
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51
128
TeTe
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127 I
Iodi
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131
Xe Xen
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137
Ba
Bar
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56
139
LaLa
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*
178
Hf
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72
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TaTa
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184 W
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186
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75
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Os
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76
192
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195 Pt
Pla
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78
197
Au
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Hg
Mer
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80
204 Tl
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81
207
Pb Lead
82
209 Bi
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PoP
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84
At
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Rn
Rad
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FrFr
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9 Be
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55
226
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Rad
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88
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READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.Write in dark blue or black pen.You may use a pencil for any diagrams, graphs or rough working.Do not use staples, paper clips, highlighters, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.
Answer all questions.Electronic calculators may be used.Practical notes are provided on page 8.You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.
CHEMISTRY 0620/51
Paper 5 Practical Test October/November 2013
1 hour 15 minutes
Candidates answer on the Question Paper.
Additional Materials: As listed in the Confi dential Instructions
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONSInternational General Certifi cate of Secondary Education
This document consists of 7 printed pages and 1 blank page.
[Turn overIB13 11_0620_51/2RP© UCLES 2013
*1146292889*
For Examiner’s Use
Total
2
0620/51/O/N/13© UCLES 2013
ForExaminer’s
Use
1 You are going to investigate what happens when aqueous sodium hydroxide reacts with acid K.
Read all the instructions below carefully before starting the experiments.
Instructions You are going to carry out two experiments.
(a) Experiment 1
Use a measuring cylinder to pour 25 cm3 of acid K into a conical fl ask. Add fi ve drops of phenolphthalein to the fl ask.
Fill the burette with the aqueous sodium hydroxide to the 0.0 cm3 mark. Slowly add the aqueous sodium hydroxide to acid K in the fl ask and shake the mixture. Continue to add aqueous sodium hydroxide to the fl ask until the solution shows a
permanent colour change. Measure and record the volume in the table. Complete the table. Pour the solution away and rinse the conical fl ask.
burette reading
fi nal volume / cm3
initial volume / cm3
difference / cm3
[3]
(b) Experiment 2
Use a measuring cylinder to pour 50 cm3 of acid K into a conical fl ask. Add the 0.3 g of powdered calcium carbonate to the fl ask and shake the fl ask until no further reaction is observed.
Add fi ve drops of phenolphthalein to the mixture in the fl ask.
Fill the burette with aqueous sodium hydroxide and record the burette reading. Slowly add aqueous sodium hydroxide from the burette to the fl ask and shake the mixture. Continue to add aqueous sodium hydroxide to the fl ask until the solution shows a permanent colour change.
Measure and record the volume in the table. Complete the table.
burette reading
fi nal volume / cm3
initial volume / cm3
difference / cm3
[3]
3
0620/51/O/N/13© UCLES 2013 [Turn over
ForExaminer’s
Use
(c) What colour change was observed after the sodium hydroxide solution was added to the fl ask?
from ............................................................ to ............................................................ [2]
(d) What type of chemical reaction occurs when acid K reacts with sodium hydroxide?
..................................................................................................................................... [1]
(e) If Experiment 1 was repeated using 50 cm3 of acid K, what volume of sodium hydroxide would be required to change the colour of the indicator?
..................................................................................................................................... [2]
(f) (i) What is the effect of adding 0.3 g of powdered calcium carbonate to acid K?
....................................................................................................................................
.............................................................................................................................. [2]
(ii) Use your answers from (b) and (e) to work out the difference in the volume of sodium hydroxide added when 0.3 g of calcium carbonate is mixed with 50 cm3 of acid K in Experiment 2.
....................................................................................................................................
.............................................................................................................................. [2]
(iii) Estimate the mass of calcium carbonate that would need to be added to 50 cm3 of acid K to require 0.0 cm3 of sodium hydroxide.
[1]
(g) What would be the effect on the results if the solutions of acid K were warmed before adding the sodium hydroxide? Give a reason for your answer.
effect on results ................................................................................................................
reason ......................................................................................................................... [2]
4
0620/51/O/N/13© UCLES 2013
ForExaminer’s
Use
(h) Suggest the advantage, if any, of
(i) using a pipette to measure the volume of acid K.
....................................................................................................................................
.............................................................................................................................. [2]
(ii) using a polystyrene cup instead of a fl ask.
....................................................................................................................................
.............................................................................................................................. [2]
[Total: 22]
5
0620/51/O/N/13© UCLES 2013 [Turn over
ForExaminer’s
Use
2 You are provided with two liquids, L and M. Carry out the following tests on L and M, recording all of your observations in the table. Conclusions must not be written in the table.
tests observationstests on liquid L
(a) Describe the appearance of liquid L. ................................................................ [1]
Divide liquid L into fi ve equal portions in separate test-tubes.
(b) (i) Add the fi rst portion of liquid L to the test-tube containing the iodine crystal. Stopper the test-tube and shake the contents.
Now add an equal volume of liquid M to the test-tube, stopper and shake the contents. Leave to stand for fi ve minutes and continue to part (c).
(ii) After fi ve minutes, remove most of the top layer using a teat pipette and add ethanol to the liquid which you have removed. Stopper the test-tube and shake the contents. Leave to stand for fi ve minutes.
................................................................ [1]
......................................................................
................................................................ [2]
......................................................................
................................................................ [2]
(c) To the second portion of liquid L, add a few drops of dilute nitric acid and about 1 cm3 of barium nitrate solution. ................................................................ [1]
(d) To the third portion of liquid L, add a few drops of dilute nitric acid and about 1 cm3 of silver nitrate solution. ................................................................ [2]
(e) To the fourth portion of liquid L, add about 1 cm3 of aqueous copper sulfate, shake and leave to stand for fi ve minutes.
......................................................................
................................................................ [2]
(f) To the fi fth portion of liquid L, add about 2 cm3 of aqueous hydrogen peroxide.
Now add about 1 cm3 of starch solution.
......................................................................
................................................................ [3]
6
0620/51/O/N/13© UCLES 2013
ForExaminer’s
Use
(g) Why does the colour of liquid L change in test (b)(i)?
...........................................................................................................................................
..................................................................................................................................... [1]
(h) What conclusions can you draw about liquid M from test (b)(i)?
...........................................................................................................................................
..................................................................................................................................... [2]
(i) What conclusions can you draw about liquid L?
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [1]
[Total: 18]
7
0620/51/O/N/13
BLANK PAGE
© UCLES 2013
8
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Everyreasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included the publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
0620/51/O/N/13
NOTES FOR USE IN QUALITATIVE ANALYSIS
Test for anions
anion test test result
carbonate (CO32–) add dilute acid effervescence, carbon dioxide
produced
chloride (Cl –)[in solution]
acidify with dilute nitric acid, thenadd aqueous silver nitrate
white ppt.
iodide (I–)[in solution]
acidify with dilute nitric acid, thenadd aqueous silver nitrate
yellow ppt.
nitrate (NO3–)
[in solution]add aqueous sodium hydroxidethen aluminium foil; warm carefully
ammonia produced
sulfate (SO42–)
[in solution]acidify with dilute nitric acid, thenaqueous barium nitrate
white ppt.
Test for aqueous cations
cation effect of aqueous sodium hydroxide effect of aqueous ammonia
aluminium (Al 3+) white ppt., soluble in excess givinga colourless solution
white ppt., insoluble in excess
ammonium (NH4+) ammonia produced on warming –
calcium (Ca2+) white ppt., insoluble in excess no ppt., or very slight white ppt.
copper (Cu2+) light blue ppt., insoluble in excess light blue ppt., soluble in excessgiving a dark blue solution
iron(II) (Fe2+) green ppt., insoluble in excess green ppt., insoluble in excess
iron(III) (Fe3+) red-brown ppt., insoluble in excess red-brown ppt., insoluble in excess
zinc (Zn2+) white ppt., soluble in excess givinga colourless solution
white ppt., soluble in excess givinga colourless solution
Test for gases
gas test and test results
ammonia (NH3) turns damp red litmus paper blue
carbon dioxide (CO2) turns limewater milky
chlorine (Cl 2) bleaches damp litmus paper
hydrogen (H2) ‘pops’ with a lighted splint
oxygen (O2) relights a glowing splint
© UCLES 2013
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.Write in dark blue or black pen.You may use a pencil for any diagrams, graphs or rough working.Do not use staples, paper clips, highlighters, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.
Answer all questions.Electronic calculators may be used.Practical notes are provided on page 8.You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.
CHEMISTRY 0620/52
Paper 5 Practical Test October/November 2013
1 hour 15 minutes
Candidates answer on the Question Paper.
Additional Materials: As listed in the Confi dential Instructions
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONSInternational General Certifi cate of Secondary Education
This document consists of 7 printed pages and 1 blank page.
[Turn overIB13 11_0620_52/FP© UCLES 2013
*6686368564*
For Examiner’s Use
Total
2
0620/52/O/N/13© UCLES 2013
ForExaminer’s
Use
1 You are going to investigate what happens when aqueous sodium hydroxide reacts with acid K.
Read all the instructions below carefully before starting the experiments.
Instructions You are going to carry out two experiments.
(a) Experiment 1
Use a measuring cylinder to pour 25 cm3 of acid K into a conical fl ask. Add fi ve drops of phenolphthalein to the fl ask.
Fill the burette with the aqueous sodium hydroxide to the 0.0 cm3 mark. Slowly add the aqueous sodium hydroxide to acid K in the fl ask and shake the mixture. Continue to add aqueous sodium hydroxide to the fl ask until the solution shows a
permanent colour change. Measure and record the volume in the table. Complete the table. Pour the solution away and rinse the conical fl ask.
burette reading
fi nal volume / cm3
initial volume / cm3
difference / cm3
[3]
(b) Experiment 2
Use a measuring cylinder to pour 50 cm3 of acid K into a conical fl ask. Add the 0.3 g of powdered calcium carbonate to the fl ask and shake the fl ask until no further reaction is observed.
Add fi ve drops of phenolphthalein to the mixture in the fl ask.
Fill the burette with aqueous sodium hydroxide and record the burette reading. Slowly add aqueous sodium hydroxide from the burette to the fl ask and shake the mixture. Continue to add aqueous sodium hydroxide to the fl ask until the solution shows a permanent colour change.
Measure and record the volume in the table. Complete the table.
burette reading
fi nal volume / cm3
initial volume / cm3
difference / cm3
[3]
3
0620/52/O/N/13© UCLES 2013 [Turn over
ForExaminer’s
Use
(c) What colour change was observed after the sodium hydroxide solution was added to the fl ask?
from ............................................................ to ............................................................ [2]
(d) What type of chemical reaction occurs when acid K reacts with sodium hydroxide?
..................................................................................................................................... [1]
(e) If Experiment 1 was repeated using 50 cm3 of acid K, what volume of sodium hydroxide would be required to change the colour of the indicator?
..................................................................................................................................... [2]
(f) (i) What is the effect of adding 0.3 g of powdered calcium carbonate to acid K?
....................................................................................................................................
.............................................................................................................................. [2]
(ii) Use your answers from (b) and (e) to work out the difference in the volume of sodium hydroxide added when 0.3 g of calcium carbonate is mixed with 50 cm3 of acid K in Experiment 2.
....................................................................................................................................
.............................................................................................................................. [2]
(iii) Estimate the mass of calcium carbonate that would need to be added to 50 cm3 of acid K to require 0.0 cm3 of sodium hydroxide.
[1]
(g) What would be the effect on the results if the solutions of acid K were warmed before adding the sodium hydroxide? Give a reason for your answer.
effect on results ................................................................................................................
reason ......................................................................................................................... [2]
4
0620/52/O/N/13© UCLES 2013
ForExaminer’s
Use
(h) Suggest the advantage, if any, of
(i) using a pipette to measure the volume of acid K.
....................................................................................................................................
.............................................................................................................................. [2]
(ii) using a polystyrene cup instead of a fl ask.
....................................................................................................................................
.............................................................................................................................. [2]
[Total: 22]
5
0620/52/O/N/13© UCLES 2013 [Turn over
ForExaminer’s
Use
2 You are provided with two liquids, L and M. Carry out the following tests on L and M, recording all of your observations in the table. Conclusions must not be written in the table.
tests observationstests on liquid L
(a) Describe the appearance of liquid L. ................................................................ [1]
Divide liquid L into fi ve equal portions in separate test-tubes.
(b) (i) Add the fi rst portion of liquid L to the test-tube containing the iodine crystal. Stopper the test-tube and shake the contents.
Now add an equal volume of liquid M to the test-tube, stopper and shake the contents. Leave to stand for fi ve minutes and continue to part (c).
(ii) After fi ve minutes, remove most of the top layer using a teat pipette and add ethanol to the liquid which you have removed. Stopper the test-tube and shake the contents. Leave to stand for fi ve minutes.
................................................................ [1]
......................................................................
................................................................ [2]
......................................................................
................................................................ [2]
(c) To the second portion of liquid L, add a few drops of dilute nitric acid and about 1 cm3 of barium nitrate solution. ................................................................ [1]
(d) To the third portion of liquid L, add a few drops of dilute nitric acid and about 1 cm3 of silver nitrate solution. ................................................................ [2]
(e) To the fourth portion of liquid L, add about 1 cm3 of aqueous copper sulfate, shake and leave to stand for fi ve minutes.
......................................................................
................................................................ [2]
(f) To the fi fth portion of liquid L, add about 2 cm3 of aqueous hydrogen peroxide.
Now add about 1 cm3 of starch solution.
......................................................................
................................................................ [3]
6
0620/52/O/N/13© UCLES 2013
ForExaminer’s
Use
(g) Why does the colour of liquid L change in test (b)(i)?
...........................................................................................................................................
..................................................................................................................................... [1]
(h) What conclusions can you draw about liquid M from test (b)(i)?
...........................................................................................................................................
..................................................................................................................................... [2]
(i) What conclusions can you draw about liquid L?
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [1]
[Total: 18]
7
0620/52/O/N/13
BLANK PAGE
© UCLES 2013
8
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Everyreasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included the publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
0620/52/O/N/13
NOTES FOR USE IN QUALITATIVE ANALYSIS
Test for anions
anion test test result
carbonate (CO32–) add dilute acid effervescence, carbon dioxide
produced
chloride (Cl –)[in solution]
acidify with dilute nitric acid, thenadd aqueous silver nitrate
white ppt.
iodide (I–)[in solution]
acidify with dilute nitric acid, thenadd aqueous silver nitrate
yellow ppt.
nitrate (NO3–)
[in solution]add aqueous sodium hydroxidethen aluminium foil; warm carefully
ammonia produced
sulfate (SO42–)
[in solution]acidify with dilute nitric acid, thenaqueous barium nitrate
white ppt.
Test for aqueous cations
cation effect of aqueous sodium hydroxide effect of aqueous ammonia
aluminium (Al 3+) white ppt., soluble in excess givinga colourless solution
white ppt., insoluble in excess
ammonium (NH4+) ammonia produced on warming –
calcium (Ca2+) white ppt., insoluble in excess no ppt., or very slight white ppt.
copper (Cu2+) light blue ppt., insoluble in excess light blue ppt., soluble in excessgiving a dark blue solution
iron(II) (Fe2+) green ppt., insoluble in excess green ppt., insoluble in excess
iron(III) (Fe3+) red-brown ppt., insoluble in excess red-brown ppt., insoluble in excess
zinc (Zn2+) white ppt., soluble in excess givinga colourless solution
white ppt., soluble in excess givinga colourless solution
Test for gases
gas test and test results
ammonia (NH3) turns damp red litmus paper blue
carbon dioxide (CO2) turns limewater milky
chlorine (Cl 2) bleaches damp litmus paper
hydrogen (H2) ‘pops’ with a lighted splint
oxygen (O2) relights a glowing splint
© UCLES 2013
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.Write in dark blue or black pen.You may use a pencil for any diagrams, graphs or rough working.Do not use staples, paper clips, highlighters, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.
Answer all questions.Electronic calculators may be used.Practical notes are provided on page 8.You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.
CHEMISTRY 0620/53
Paper 5 Practical Test October/November 2013
1 hour 15 minutes
Candidates answer on the Question Paper.
Additional Materials: As listed in the Confi dential Instructions
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONSInternational General Certifi cate of Secondary Education
This document consists of 6 printed pages and 2 blank pages.
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0620/53/O/N/13© UCLES 2013
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1 You are going to investigate the reaction between aqueous potassium manganate(VII), solution C, and two different acidic solutions, D and E.
Read all the instructions below carefully before starting the experiments.
Instructions You are going to carry out three experiments.
(a) Experiment 1
Fill the burette with the solution C of potassium manganate(VII) to the 0.0 cm3 mark. Using a measuring cylinder, pour 25 cm3 of solution D into the conical fl ask.
Add 1.0 cm3 of the solution C to the fl ask, with shaking. Continue to add solution C to the fl ask until the mixture just turns permanently pink. Record the burette reading in the table and complete the table.
Pour away the contents of the conical fl ask and rinse the fl ask with distilled water.
burette reading
fi nal burette reading / cm3
initial burette reading / cm3
difference / cm3
[3]
(b) Experiment 2
Repeat Experiment 1 using 25 cm3 of solution E instead of solution D. Record the burette readings in the table and complete the table.
burette reading
fi nal burette reading / cm3
initial burette reading / cm3
difference / cm3
[3]
(c) Experiment 3
To about 2 cm3 of solution E in a test-tube, add an equal volume of aqueous ammonia. Shake the test-tube and note any observations. Leave the mixture to stand for 5 minutes and note any changes.
...........................................................................................................................................
..................................................................................................................................... [2]
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(d) (i) What colour change was observed as potassium manganate(VII) solution was added to the fl ask in Experiment 1?
................................................................................................................................[1]
(ii) Why is an indicator not added to the fl ask?
.............................................................................................................................. [1]
(e) (i) In which experiment was the greatest volume of potassium manganate(VII) solution used?
.............................................................................................................................. [1]
(ii) Compare the volumes of potassium manganate(VII) used in Experiments 1 and 2.
.............................................................................................................................. [1]
(iii) Suggest an explanation for the difference in volumes.
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [2]
(f) If Experiment 2 was repeated using 12.5 cm3 of solution E, what volume of potassium manganate(VII) solution would be used? Explain your answer.
...........................................................................................................................................
..................................................................................................................................... [2]
(g) Give one advantage and one disadvantage of using a measuring cylinder for solutions D and E.
advantage .........................................................................................................................
disadvantage ............................................................................................................... [2]
(h) Explain your observations in Experiment 3.
...........................................................................................................................................
..................................................................................................................................... [3]
[Total: 21]
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2 You are provided with liquid F. Carry out the following tests on the liquid, recording all of your observations in the table. Conclusions must not be written in the table.
tests observations
Divide liquid F into fi ve equal portions in separate test-tubes.
(a) Describe the appearance of liquid F.
Test the pH of the liquid.
To the fi rst portion of liquid F, add an equal volume of dilute sulfuric acid.
Now add excess aqueous sodium hydroxide and shake the mixture.
................................................................ [1]
................................................................ [1]
......................................................................
................................................................ [2]
(b) To the second portion of liquid F, add an equal volume of dilute sulfuric acid followed by about 2 cm3 of hydrogen peroxide.
Shake the mixture and test the gas given off with a splint.
......................................................................
................................................................ [1]
................................................................ [2]
(c) To the third portion of liquid F, add aqueous silver nitrate followed by excess dilute nitric acid. Shake the mixture.
......................................................................
................................................................ [3]
(d) To the fourth portion of liquid F, add aqueous barium nitrate followed by excess dilute nitric acid. Shake the mixture.
......................................................................
................................................................ [3]
(e) To the fi fth portion of liquid F, add an equal volume of sulfuric acid and one spatula measure of iron fi lings.
......................................................................
................................................................ [2]
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(f) What type of reaction happened in test (a)? Explain your answer.
type of reaction .................................................................................................................
explanation .......................................................................................................................
..................................................................................................................................... [2]
(g) Identify the gas given off in test (b).
..................................................................................................................................... [1]
(h) Draw one conclusion about liquid F.
..................................................................................................................................... [1]
[Total: 19]
6
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© UCLES 2013
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Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Everyreasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included the publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
0620/53/O/N/13
NOTES FOR USE IN QUALITATIVE ANALYSIS
Test for anions
anion test test result
carbonate (CO32–) add dilute acid effervescence, carbon dioxide
produced
chloride (Cl –)[in solution]
acidify with dilute nitric acid, thenadd aqueous silver nitrate
white ppt.
iodide (I–)[in solution]
acidify with dilute nitric acid, thenadd aqueous silver nitrate
yellow ppt.
nitrate (NO3–)
[in solution]add aqueous sodium hydroxidethen aluminium foil; warm carefully
ammonia produced
sulfate (SO42–)
[in solution]acidify with dilute nitric acid, thenaqueous barium nitrate
white ppt.
Test for aqueous cations
cation effect of aqueous sodium hydroxide effect of aqueous ammonia
aluminium (Al 3+) white ppt., soluble in excess givinga colourless solution
white ppt., insoluble in excess
ammonium (NH4+) ammonia produced on warming –
calcium (Ca2+) white ppt., insoluble in excess no ppt., or very slight white ppt.
copper (Cu2+) light blue ppt., insoluble in excess light blue ppt., soluble in excessgiving a dark blue solution
iron(II) (Fe2+) green ppt., insoluble in excess green ppt., insoluble in excess
iron(III) (Fe3+) red-brown ppt., insoluble in excess red-brown ppt., insoluble in excess
zinc (Zn2+) white ppt., soluble in excess givinga colourless solution
white ppt., soluble in excess givinga colourless solution
Test for gases
gas test and test results
ammonia (NH3) turns damp red litmus paper blue
carbon dioxide (CO2) turns limewater milky
chlorine (Cl 2) bleaches damp litmus paper
hydrogen (H2) ‘pops’ with a lighted splint
oxygen (O2) relights a glowing splint
© UCLES 2013
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.Write in dark blue or black pen.You may use a pencil for any diagrams, graphs or rough working.Do not use staples, paper clips, highlighters, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.
Answer all questions.Electronic calculators may be used.You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.
CHEMISTRY 0620/61
Paper 6 Alternative to Practical October/November 2013
1 hour
Candidates answer on the Question Paper.
No Additional Materials are required.
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONSInternational General Certifi cate of Secondary Education
This document consists of 10 printed pages and 2 blank pages.
[Turn overIB13 11_0620_61/2RP© UCLES 2013
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1 A student investigated the products formed when ethanol was burned using the apparatus shown.
suctionpump
liquid F
(a) Complete the box to identify the piece of apparatus. [1]
(b) Why is a suction pump used?
..................................................................................................................................... [1]
(c) (i) Suggest the purpose and identity of liquid F.
identity .......................................................................................................................
purpose ................................................................................................................ [2]
(ii) Why is the end of the delivery tube below the surface of liquid F?
....................................................................................................................................
.............................................................................................................................. [1]
(d) Give one expected observation in the horizontal part of the delivery tube. Explain your answer.
...........................................................................................................................................
..................................................................................................................................... [2]
[Total: 7]
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2 Eight steel rods of the same size were placed in solutions of different pH for one week. The percentage corrosion of the rods was measured and the results plotted on the grid below.
30
20
10
0
perc
enta
ge c
orro
sion
of s
teel
rod
0 1 2 3 4pH of solution
5 6 7 8
(a) Draw a best fi t straight line through the points. [1]
(b) Why were the steel rods the same size?
..................................................................................................................................... [1]
(c) State one other variable which should have been kept constant.
..................................................................................................................................... [1]
(d) State one conclusion that could be drawn from the results.
..................................................................................................................................... [1]
(e) Determine the percentage corrosion of a steel rod in a solution of pH 6.5.
..................................................................................................................................... [1]
[Total: 5]
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3 A student investigated the reaction between aqueous sodium hydroxide and acid K. Two experiments were carried out.
(a) Experiment 1
Using a measuring cylinder, 25 cm3 of acid K was poured into a conical fl ask. Phenolphthalein indicator was added to the fl ask. A burette was fi lled with aqueous sodium hydroxide to the 0.0 cm3 mark. Aqueous sodium hydroxide was added from the burette to the fl ask and the mixture shaken until the solution showed a permanent colour change.
The fi nal volume was measured. Use the burette diagram to record the fi nal volume in the table and complete the table.
37
38
39
final volume
burette reading
final volume / cm3
initial volume / cm3
difference / cm3
[2]
(b) Experiment 2
The solution was poured away and the conical fl ask rinsed. Using a measuring cylinder, 50 cm3 of acid K was poured into the conical fl ask. 0.3 g of
powdered calcium carbonate was added to the fl ask and the fl ask shaken until no further reaction was observed.
Phenolphthalein was added to the mixture in the fl ask. A burette was fi lled with the same aqueous sodium hydroxide and the initial volume
measured. Aqueous sodium hydroxide was added from the burette to the fl ask and the mixture shaken until the solution showed a permanent colour change.
Use the burette diagrams to record the initial and fi nal volumes in the table and complete the table.
initial volume final volume
28
29
30
9
10
11
burette reading
final volume / cm3
initial volume / cm3
difference / cm3
[2]
5
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(c) What colour change was observed after the sodium hydroxide solution was added to the fl ask?
from ............................................................ to ............................................................ [2]
(d) What type of chemical reaction occurred when acid K reacted with sodium hydroxide?
..................................................................................................................................... [1]
(e) If Experiment 1 were repeated using 50 cm3 of acid K, what volume of sodium hydroxide would be required to change the colour of the indicator?
..................................................................................................................................... [2]
(f) (i) What were the effects of adding 0.3 g of powdered calcium carbonate to acid K?
....................................................................................................................................
.............................................................................................................................. [2]
(ii) Use your answer in (e) to work out the difference between the volume of sodium hydroxide needed to completely react with 50 cm3 of acid K and the volume of sodium hydroxide used in Experiment 2.
....................................................................................................................................
.............................................................................................................................. [2]
(iii) Estimate the mass of calcium carbonate that would be needed to be added to 50 cm3 of acid K to require 0.0 cm3 of sodium hydroxide.
.............................................................................................................................. [1]
(g) What would be the effect on the results if the solutions of acid K were warmed before adding the sodium hydroxide? Give a reason for your answer.
effect on results ................................................................................................................
reason ......................................................................................................................... [2]
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(h) Suggest the advantage, if any, of
(i) using a pipette to measure the volume of acid K.
....................................................................................................................................
.............................................................................................................................. [2]
(ii) using a polystyrene cup instead of a fl ask.
....................................................................................................................................
.............................................................................................................................. [2]
[Total: 20]
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4 Two liquids, L and M, were analysed. L was aqueous potassium iodide. M was a colourless liquid.
The tests on the liquids and some of the observations are in the following table. Complete the observations in the table.
tests observations
tests on liquid L
(a) Appearance of liquid L. ............................................................ [1]
Liquid L was divided into three equal portions in separate test-tubes.
(b) (i) An iodine crystal was added to the fi rst portion of liquid L. The test-tube was stoppered and the contents shaken.
(ii) An equal volume of liquid M was added to the test-tube, the contents shaken and left to stand for fi ve minutes.
liquid turned orange
two layers were formed,pink top layer and orange lower layer
(c) To the second portion of liquid L, dilute nitric acid and barium nitrate solution were added. ............................................................ [1]
(d) To the third portion of liquid L, dilute nitric acid and silver nitrate solution were added. ............................................................ [2]
(e) Why does the colour of liquid L change in test (b)(i)?
...........................................................................................................................................
..................................................................................................................................... [1]
(f) What conclusions can you draw about liquid M from test (b)(ii)?
...........................................................................................................................................
..................................................................................................................................... [2]
[Total: 7]
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5 Two experiments using catalysts were carried out. Catalysts R and S were used to break down 50 cm3 of aqueous hydrogen peroxide at a temperature of 20 °C. The volume of oxygen given off was measured using the apparatus shown.
aqueoushydrogen peroxide
catalyst
gas syringe
The gas syringe diagrams show the volume of oxygen formed every 30 seconds in each experiment.
(a) Use the syringe diagrams to complete the volumes in the table.
time / s syringe diagram
using catalyst R using catalyst S
volume / cm3 syringe diagram volume / cm3
0 100
20 30 40
30 40 50
50 60 70
60 70 80
60 70 80
60 70 80
0 10
10 20 30
30 40 50
50 60 70
60 70 80
60 70 80
60 70 80
30
60
90
120
150
180
[4]
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(b) Plot a graph to show each set of results. Clearly label the graphs R and S.
80
70
60
50
40
30
20
10
0
volume ofoxygen / cm3
0 30 60 90 120time / s
150 180
[6]
(c) Which result using catalyst R was inaccurate?
..................................................................................................................................... [1]
(d) Which is the better catalyst in this reaction? Explain your answer.
...........................................................................................................................................
..................................................................................................................................... [2]
(e) Sketch a line on the grid to show the graph you would expect if the reaction with catalyst R was repeated at 50 °C. [2]
[Total: 15]
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6Old documents
Some documents are stored in containers with packets of silica gel crystals. These crystals absorb water from air that enters the container. Water could damage the documents.
Anhydrous cobalt(II) chloride is added to the silica gel. As the crystals absorb water they change colour from blue to pink. Heating the silica gel in an oven removes the water from the crystals so that the crystals can be reused.
Plan an experiment to fi nd the mass of water absorbed by a packet of silica gel crystals.
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
............................................................................................................................................ [6]
[Total: 6]
11
0620/61/O/N/13
BLANK PAGE
© UCLES 2013
12
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Everyreasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included the publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
0620/61/O/N/13
BLANK PAGE
© UCLES 2013
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.Write in dark blue or black pen.You may use a pencil for any diagrams, graphs or rough working.Do not use staples, paper clips, highlighters, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.
Answer all questions.Electronic calculators may be used.You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.
CHEMISTRY 0620/62
Paper 6 Alternative to Practical October/November 2013
1 hour
Candidates answer on the Question Paper.
No Additional Materials are required.
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONSInternational General Certifi cate of Secondary Education
This document consists of 12 printed pages.
[Turn overIB13 11_0620_62/2RP© UCLES 2013
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1 Alkenes can be made by cracking long chain alkanes. A student used the apparatus below to demonstrate cracking.
broken tileliquid alkane
on mineral wool
very strongheat
water
(a) Complete the box to show the apparatus used. [1]
(b) Indicate with an arrow where the alkenes are collected. [1]
(c) Suggest the purpose of the mineral wool.
..................................................................................................................................... [1]
(d) Why are small pieces of broken tile used?
...........................................................................................................................................
..................................................................................................................................... [1]
(e) Describe a test to show that alkenes have been made.
test ....................................................................................................................................
result ........................................................................................................................... [2]
[Total: 6]
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2 Substance M is a mixture of four dyes. Three of the dyes have different solubilities in propanone. The fourth dye is insoluble in propanone.
(a) Name the process that could be used to separate these dyes.
..................................................................................................................................... [1]
(b) Sketch on the right hand diagram the results you would expect if M was analysed as shown.
base-line
propanoneat the beginning at the end
M
[2]
(c) Why is the base-line not drawn in ink?
...........................................................................................................................................
..................................................................................................................................... [1]
(d) Why must the level of the propanone be below the base-line?
..................................................................................................................................... [1]
[Total: 5]
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3 A student investigated the formation of calcium oxide by heating calcium in air, using the apparatus shown.
heat
crucible
She weighed an empty crucible and its lid. She then added some calcium to the crucible and reweighed it.
(a) Use the balance diagrams to record the masses in the table.
balance diagram mass / g
mass of crucible and lid
32
31
mass of crucible, lid and calcium
32
31
[1]
The student then heated the calcium in the crucible for ten minutes. The lid was raised occasionally using a pair of tongs. After ten minutes, the crucible was allowed to cool and reweighed. This procedure was repeated twice.
(b) Use the balance diagrams to complete the table of results.
time / min 10 20 30
balance diagram
32
31
33
32
33
32
mass of crucible, lid and calcium oxide / g
[2]
5
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(c) Why was the lid of the crucible raised occasionally?
..................................................................................................................................... [1]
(d) Explain why the crucible was heated three times.
...........................................................................................................................................
..................................................................................................................................... [2]
The table shows the results of experiments using different masses of calcium.
experiment mass ofcalcium / g
mass ofcalcium oxide / g
mass ofoxygen reacted / g
1 0.12 0.20 0.08
2 0.20 0.32 0.12
3 0.30 0.49 0.19
4 0.40 0.61
5 0.44 0.72
6 0.48 0.79
7 0.56 0.92
(e) Complete the table of results. [1]
(f) Plot the results on the grid and draw a straight line graph.
0.5
0.4
0.3
0.2
0.1
0.00.0 0.1 0.2 0.3 0.4
mass of calcium / g0.5 0.6 0.7
mas
s of
oxy
gen
reac
ted
/ g
[5]
6
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(g) Which result is inaccurate?
..................................................................................................................................... [1]
(h) Use your graph to work out the mass of calcium oxide formed when 0.7 g of calcium is heated in air. Show clearly on the grid how you used your graph.
[3]
[Total: 16]
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4 A student investigated what happened when dilute hydrochloric acid and aqueous copper(II) sulfate solution reacted with different metals.
Five experiments were carried out.
(a) Experiment 1
Using a measuring cylinder 10 cm3 of dilute hydrochloric acid was poured into a boiling tube. The temperature of the solution was measured.
1 g of zinc powder was added to the boiling tube and the mixture stirred with the thermometer. The maximum temperature of the mixture was measured.
(b) Experiment 2
Experiment 1 was repeated using 1 g of iron powder instead of zinc. The initial and maximum temperatures were measured.
(c) Experiment 3
Experiment 1 was repeated using 1 g of magnesium powder instead of zinc. The initial and maximum temperatures were measured.
Use the thermometer diagrams to record the temperatures in the table. Complete the table.
experiment thermometer diagram
initialtemperature / °C
thermometer diagram
maximumtemperature / °C
temperaturerise / °C
1
30
25
20
30
25
20
2
30
25
20
30
25
20
3
30
25
20
80
75
70
[3] (d) Experiment 4
Using a measuring cylinder, 10 cm3 of aqueous copper sulfate was poured into a boiling tube. The temperature of the solution was measured.
1 g of magnesium powder was added to the boiling tube and the mixture stirred with the thermometer.
The gas was tested with a lighted splint and a loud pop was observed. The maximum temperature of the mixture was measured.
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(e) Experiment 5
Experiment 4 was repeated using 1 g of iron powder instead of magnesium. A red-brown solid was formed.
Use the thermometer diagrams to record the temperatures in the table. Complete the table.
experiment thermometer diagram
initialtemperature / °C
thermometer diagram
maximumtemperature / °C
temperaturerise / °C
4
5
[3]
(f) Draw a labelled bar chart for the results of Experiments 1, 2, 3, 4 and 5 on the grid below.
temperaturerise / °C
[5]
9
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Use the results and observations to answer the following questions.
(g) (i) Which Experiment produced the largest temperature rise?
.............................................................................................................................. [1]
(ii) Suggest why this Experiment produced the largest temperature rise.
.............................................................................................................................. [1]
(h) Name the gas given off in Experiment 4.
..................................................................................................................................... [1]
(i) (i) Identify the red-brown solid formed in Experiment 5.
.............................................................................................................................. [1]
(ii) What type of chemical reaction occurs when iron reacts with aqueous copper(II) sulfate in Experiment 5?
.............................................................................................................................. [1]
(j) Predict the effect on the temperature change if 1 g of magnesium ribbon was used in Experiment 3. Explain your answer.
effect .................................................................................................................................
explanation .......................................................................................................................
..................................................................................................................................... [2]
(k) Suggest why potassium was not used as one of the metals in these experiments.
...........................................................................................................................................
..................................................................................................................................... [1]
[Total: 19]
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5 Two different liquids, A and B, were analysed. A was an aqueous solution of ethanoic acid and B was a pure liquid. The tests on the liquids and some of the observations are in the following table. Complete the observations in the table.
tests observations
tests on liquid A
Liquid A was divided into three equal portions in separate test-tubes.
(a) Colour and smell of liquid A.
The liquid was added to Universal Indicator.
................................................................ [1]
colour changed from green to ......................
pH .......................................................... [2]
(b) A piece of magnesium ribbon was added to the second portion of liquid A.
The gas given off was tested with a splint.
......................................................................
......................................................................
................................................................ [3]
(c) Calcium carbonate was added to the third portion of liquid A. ................................................................ [1]
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Usetests observations
tests on liquid B
(d) Dilute sulfuric acid was added to liquid B followed by aqueous potassium manganate(VII). The mixture was heated.
changed colour from purple to colourless
(e) Liquid B was poured onto a dry watch glass. The surface of the liquid was touched with a lighted splint.
liquid burned with a yellow / blue fl ame
(f) What conclusions can you draw about liquid B?
...........................................................................................................................................
..................................................................................................................................... [2]
[Total: 9]
12
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Everyreasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included the publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
0620/62/O/N/13© UCLES 2013
ForExaminer’s
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6Hair bleach
A solution of hydrogen peroxide can be used to bleach hair. Hairdressers buy ‘20 volume’ hydrogen peroxide. One volume of this solution breaks down to form 20 volumes of oxygen. For example 10 cm3 of 20 volume hydrogen peroxide will break down to produce 200 cm3 of oxygen.
Old solutions of hydrogen peroxide will produce less oxygen than expected.
Plan an experiment to fi nd out which of two solutions of hydrogen peroxide, H and J, is new and which is old. You are provided with common laboratory apparatus and the catalyst manganese(IV) oxide which speeds up the break down of hydrogen peroxide.
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
............................................................................................................................................ [5]
[Total: 5]
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.Write in dark blue or black pen.You may use a pencil for any diagrams, graphs or rough working.Do not use staples, paper clips, highlighters, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.
Answer all questions.Electronic calculators may be used.You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.
CHEMISTRY 0620/63
Paper 6 Alternative to Practical October/November 2013
1 hour
Candidates answer on the Question Paper.
No Additional Materials are required.
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONSInternational General Certifi cate of Secondary Education
This document consists of 9 printed pages and 3 blank pages.
[Turn overIB13 11_0620_63/RP© UCLES 2013
*8630438523*
2
0620/63/O/N/13© UCLES 2013
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1 A student tried to separate a mixture of salt and sand. Salt, sodium chloride, is soluble in water. Sand, silicon(IV) oxide, is insoluble in water. He added the mixture to water. Three sets of apparatus are shown.
A B C
(a) Complete the boxes to identify the pieces of apparatus. [2]
(b) Fill in the blanks in the following sentences.
Liquids that dissolve substances are called ........................ .
The clear liquid formed is a ................................. . [2]
(c) Which set of apparatus should be used to obtain
the sand, ...................................
salt crystals? ............................. [2]
(d) What happened to the water used in the experiment?
..................................................................................................................................... [1]
[Total: 7]
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2 Sulfur dioxide is a poisonous gas which is denser than air and soluble in water. Sulfur dioxide can be prepared by adding dilute hydrochloric acid to sodium sulfi te and
warming the mixture. Study the diagram of the apparatus used.
hydrochloricacid
sodium sulfite water
heat
(a) Identify and explain three mistakes in the diagram.
1 mistake ........................................................................................................................
reason .................................................................................................................... [2]
2 mistake ........................................................................................................................
reason .................................................................................................................... [2]
3 mistake ........................................................................................................................
reason .................................................................................................................... [2]
(b) State one precaution that should be taken when carrying out this experiment.
..................................................................................................................................... [1]
[Total: 7]
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3 A scientist measured the boiling point of water at different pressures.
(a) Use the thermometer diagrams in the table to complete the boiling point temperatures.
pressure/ atmospheres
thermometerdiagram
boiling point/ °C
1
105
100
95
2
125
120
115
3
140
135
130
4
140
135
130
5
155
150
145
6
160
155
150
7
170
165
160
[3]
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(b) Plot the points on the grid and draw a smooth line graph.
170
160
150
140
130
120
110
1000 1 2 3 4
pressure / atmospheres
5 6 7 8
boili
ng p
oint
/ °C
[4]
(c) State which point is inaccurate. Why have you chosen this point?
...........................................................................................................................................
..................................................................................................................................... [2]
(d) Use your graph to fi nd the boiling point of water at a pressure of 7.5 atmospheres. Show clearly on the grid how you obtained your answer.
..................................................................................................................................... [3]
(e) State a chemical test for water.
test ....................................................................................................................................
result ........................................................................................................................... [2]
[Total: 14]
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4 A student investigated the reaction between aqueous potassium manganate(VII), which is purple, and two different colourless acidic solutions, D and E.
Three experiments were carried out.
(a) Experiment 1
A burette was fi lled with the solution of potassium manganate(VII) to the 0.0 cm3 mark. Using a measuring cylinder, 25 cm3 of solution D was poured into a conical fl ask.
Potassium manganate(VII) solution was added to the fl ask until the mixture just turned permanently pink.
Use the burette diagram to record the fi nal volume in the table and complete the table.
14
15
16
final reading
burette reading
fi nal burette reading / cm3
initial burette reading / cm3
difference / cm3
[2]
(b) Experiment 2
Experiment 1 was repeated using 25 cm3 of solution E instead of solution D.
Use the burette diagrams to record the readings in the table and complete the table.
15
16
27
initial reading
46
47
48
final reading
burette reading
fi nal burette reading / cm3
initial burette reading / cm3
difference / cm3
[2]
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(c) Experiment 3
Aqueous ammonia was added to solution E in a test-tube. A green precipitate was observed.
The mixture was left to stand for 5 minutes. The surface of the precipitate turned brown.
What conclusions can you draw from these observations?
...........................................................................................................................................
..................................................................................................................................... [3]
(d) (i) What colour change was observed as potassium manganate(VII) solution was added to the fl ask in Experiment 1?
.............................................................................................................................. [1]
(ii) Why was an indicator not added to the fl ask?
.............................................................................................................................. [1]
(e) (i) In which experiment was the greatest volume of potassium manganate(VII) solution used?
.............................................................................................................................. [1]
(ii) Compare the volumes of potassium manganate(VII) used in Experiments 1 and 2.
.............................................................................................................................. [1]
(iii) Suggest an explanation for the difference in volumes.
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [2]
(f) If Experiment 2 was repeated using 12.5 cm3 of solution E, what volume of potassium manganate(VII) solution would be used? Explain your answer.
...........................................................................................................................................
..................................................................................................................................... [2]
(g) Give one advantage and one disadvantage of using a measuring cylinder for solutions D and E.
advantage .........................................................................................................................
disadvantage .............................................................................................................. [2]
[Total: 17]
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5 Two liquids, F and G, were analysed. G was an aqueous solution of potassium chloride. The tests on the liquids and some of the observations are in the following table. Complete the observations in the table.
tests observations
tests on liquid F
(a) (i) Appearance of liquid F.
The pH of the liquid was tested.
(ii) An equal volume of dilute sulfuric acid was added to liquid F.
Excess aqueous sodium hydroxide was then added to the mixture.
yellow solution
pH = 7
solution turned orange
solution turned from orange to yellow
(b) Dilute sulfuric acid was added to liquid F followed by hydrogen peroxide.
The mixture was shaken and the gas given off tested with a splint.
rapid effervescence
glowing splint relit
tests on liquid G
(c) Dilute nitric acid was added to liquid G followed by aqueous barium nitrate. ................................................................ [1]
(d) Dilute nitric acid was added to liquid G followed by aqueous silver nitrate. ................................................................ [2]
(e) What does test (a)(i) tell you about liquid F?
...........................................................................................................................................
..................................................................................................................................... [2]
(f) What type of reaction happened in test (a)(ii)? Explain your answer.
type of reaction .................................................................................................................
explanation .......................................................................................................................
..................................................................................................................................... [2]
(g) Identify the gas given off in test (b).
..................................................................................................................................... [1]
[Total: 8]
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6Indigestion tablets
Indigestion pain is caused by too much acid in your stomach. The acid is hydrochloric acid. Indigestion tablets contain a base which neutralises the acid.
You are provided with two different brands of indigestion tablets, Painremuve and Indcure.
Plan an investigation to compare which of these brands of tablet is the most effective. You are provided with dilute hydrochloric acid and common laboratory apparatus.
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
............................................................................................................................................ [7]
[Total: 7]
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Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Everyreasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included the publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
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