2013/14

Review Packetfor

General Chemistry Final (Timberlake)Mrs. Ancell

WHAT: Chemistry Final

WHERE: Room # 283

WHEN: Tues. June 11th 7:45 – 9:15 am

WHO: Everyone

BRING: at least 2, #2 pencils (with lead!!), eraser, calculator

COVERING:7.1-7.5 Chemical Quantities9.1-9.4 Stoichiometry3.3-3.5, 9.5, 10.5 Thermochemistry12.5 Solutions and Dilutions

14.1-14.3, 14.5-14.8 Acid/ Bases9.5, 13.1-13.2, 13.5 Equilibrium/ Le Châtelier’s 11.1-11.8, 11.10 Gas Laws

TURN IN YOUR TEXTBOOK AT THE FINAL!!

This study guide is NOT intended to teach. It is, rather, intended to jog your memory so that you recall all the many topics that

were learned during the second semester. It includes questions on each section, subject, and selected labs. The results should act

as a guide to that which you already know and only need to review, that on which you are a little rusty and need to practice, and

that which you still need to master with more intensive study. Do not wait until the last minute to ‘cram’ for the final. You should

start now doing a little each night at home. Take your book and your classroom notes/ work-packets/ old labs home with you and

use them to help review and study for the final

2013-14 GenChem Final ReviewPart I: MULTIPLE CHOICE QUESTIONS:

7.1 – 7.5Chemical Quantities

1) How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C H O?A. 5 (6.02 10 ) B. 5 C. 35 D. 35 (6.02 10 )

2) Avogadro's number of representative particles is equal to one ____.A. kilogram B. gram C. kelvin D. mole

3) All of the following are equal to Avogadro's number EXCEPT ____.A. the number of atoms of bromine in 1 mol Br B. the number of atoms of gold in 1 mol Au C. the number of molecules of nitrogen in 1 mol N D. the number of molecules of CO in 1

mol CO

4) How many atoms are in 0.075 mol of titanium?A. 1.2 10-25 B. 2.2 10 C. 6.4 10 D. 4.5 10

5) How many molecules are in 2.10 mol CO ?A. 2.53 10 molecules B. 3.79 10 molecules C. 3.49 10 molecules D. 1.26 10 molecules

6) The atomic masses of any two elements contain the same number of ____.A. atoms B. grams C. ions D. milliliters

7) What is true about the molar mass of chlorine gas?A. The molar mass is 35.5 g. B. The molar mass is 71.0 g. C. The molar mass is equal to the D. none of the above mass of one mole of chlorine atoms.

8) What is the molar mass of AuCl3?A. 96 g B. 130 g C.  232.5 g D. 303.6 g

9) What is the number of moles in 432 g Ba(NO ) ?A. 0.237 mol B. 0.605 mol C. 1.65 mol D. 3.66 mol

10) What is the number of moles of beryllium atoms in 36 g of Be?

A. 0.25 mol B. 4.0 mol C. 45.0 mol D. 320 mol

11) What information is needed to calculate the percent composition of a compound?A. the weight of the sample to be analyzed and its density B. the weight of the sample to be

analyzed and its molar volume

C. the formula of the compound and the atomic mass of D. the formula of the compound and its elements density

12) What is the percent composition of chromium in BaCrO ?

A. 4.87% B. 9.47% C. 20.5% D. 25.2%

13) The lowest whole-number ratio of the elements in a compound is called the ____.A. empirical formula B. molecular formula C. binary formula D. representative formula

14) Which of the following is NOT an empirical formula?A. C N H B. C H O C. BeCr O D. Sb S

15) Which of the following compounds have the same empirical formula?A. CO and SO B. C H and C H C. C H and C H D. C H and C H

16) What is the empirical formula of a substance that is 53.5% C, 15.5% H, and 31.1% N by weight?A. C3HN2 B. C4H14N2 C. C2H7N D. CH4N7

17) The ratio of carbon atoms to hydrogen atoms to oxygen atoms in a molecule of dicyclohexyl maleate is 4 to 6

to 1. What is its molecular formula if its molar mass is 280 g?A. C H O B. C H O C. C H O D. C H O

9.1 – 9.4Reaction Stoichiometry; Limiting Reactants; Percent Yield For the questions (18 thru 21), consider the following equation.

2C2H2 (g)+ 5O2 (g) → 4CO2 (g) + 2H2O(g) acetylene

18)

If 0.500 mol of acetylene is allowed to completely react with oxygen, what is the final yield of CO2 in moles?

A)

2.00 mol

B)

4.00 mol

C)

1.00 mol

D)

0.100 mol

E)

0.500 mol

19)

If 20.0 g acetylene is allowed to completely react with oxygen, how many g of O2 are reacted?A)

9.85 g

B)

24.6 g

C)

5.00 g

D)

61.4 g

E)

20.0 g

20)

If 40.0 g of acetylene is allowed to react with 40.0 g of oxygen , how many grams of CO2 are formed?A)

135 g

B)

44.0 g

C)

40.0 g

D)

80.0 g

E)

55.0 g

21)

When 50.0 g of acetylene is allowed to react with excess oxygen, 75.0 g of CO2 are formed. What is the percent yield of carbon dioxide?

A)

100.%

B)

150.%

C)

6.7%

D)

44.4%

E)

88.8%

22)

Magnesium sulfate reacts with barium chloride according to the following balanced equation. If 1.20 g of magnesium sulfate is allowed to react with 1.00 g of barium chloride in a water solution, what is the limiting reagent?

MgSO4(aq) + BaCl2(aq) → BaSO4(s) + MgCl2(aq)

A)

magnesium chloride B)

barium chloride C)

magnesium sulfate D)

barium sulfate E)

water

3.3-3.5, 9.5, 10.5Thermochemistry

23) A solid is dissolved in a coffee cup calorimeter. Which of the following observations suggests that the process is exothermic?

A) temperature of the solution decreasesB) temperature of the solution increasesC) temperature of the solution stays the same

24) The specific heat of a substance is defined as ___.A) the energy required to raise the temperature of 1 gram of the substance by 1oCB) the energy required to vaporize 1 mole of the substance at its normal boiling pointC) the average kinetic energy of the substanceD) the energy required to raise the temperature of the entire substance by 1o

E ) the hotness or coldness of the substance

25) The following chemical equation represents what happens when solid NaOH heated.

NaOH(s) + HEAT → NaOH(l) Which of the following phrases best describes this process?

A) endothermic, heat is absorbed by the systemB) exothermic, heat is absorbed by the systemC) endothermic, heat is released by the systemD) exothermic, heat is released by the systemE) endothermic, heat is released by the surroundings

26) The graph below represents the uniform heating of a solid, starting below its melting point.

What portion of the graph shows the warming of the liquid phase of the substance?A) EF B) AB C) DE D) CD E) BC

27) What is the name of the process which occurs when a substance passes from the gas to the liquid phase?A) sublimation B) condensation C) melting D) freezing E) deposition

The following table lists the specific heats for a few substances. Use this table to answer Question 28 and 29

SubstanceSpecific Heat

( )Copper (Cu) 0.385Iron (Fe) 0.452Silver (Ag) 0.235Sodium chloride (NaCl)(s) 0.864Ammonia (NH3)(g) 2.04

28) If the same amount of heat is supplied to 10.0 g of each substance all at 21.0oC, which substance would experience the LARGEST change in temperature?

A) Cu B) Fe C) Ag D) NaCl E) NH3

29) A 25.0 g piece of copper undergoes a temperature increase of 100.0oC. How much energy, in joules, did the

copper absorb ?A) 962 J B) 2500 J C) 6490 J D) 9.63 J E) 0.0962 J

30) A solute is dissolved in water in a coffee cup calorimeter and the dissolving process results in a positive ΔHSol'n. The temperature of the resulting solution will:

A) increase B) decreaseC) stay the same

12.5Solutions/ Dilutions

31) What volume of a 3.5 M stock solution is necessary to make 100. mL of a 0.1 M dilution?A) 2.9 mL B) 35 mL C) 350 mL D) 0.35 mL E) 10. ml

32)

What is the molarity of a solution which contains 58.4 g of sodium chloride dissolved in 500 mL of solution?

A)

1.50 M B) 1.00 M C) 2.00 M D) 0.500 M E) 4.00 M

33)

How many moles of CaCl2 are in 150. mL of a 2.00 M of CaCl2 solution? A)

300. mol B) 0.300 mol C) 0.0133 mol D) 13.3 mol E) 13.3 mol

34)

How many milliliters of 2.25 M KOH solution are needed to provide 0.660 mol of KOH? A)

0.293 mL B) 2.93 mL C) 293 mL D) 29.3 mL E) 34.1 mL

35)

How many moles of CaCl2 are in 250. mL of a 3.00 M of CaCl2 solution? A) 1.33 mol B) 0.750 mol C) 83.3 mol D) 750. mol E) 3.00 mole

36) What is the molarity of 500.0 mL of a dilution made with 50.0 mL of a 2.50 M stock solution? A) 125 M B) 1 × 104 M C) 10 M D) 20 M E) 0.25 M

Chp. 14.1-14.3, 14.5-14.8 Acids and Bases

37)

The indicator phenolphthalein is ___ in acid and ___ in base.A) colorless, pink B) pink, blue C) blue, pink D) pink, colorless E) light blue, dark blue

38)

What type of reaction is shown by the chemical equation below?

HCl(aq) + NaOH(aq) → H2O(l) + NaCl (aq)

A)

single replacement B) synthesis C) neutralization D) combustion E) decomposition

39)

What is the [OH - ] in a solution with [H3O+] = 1.0 × 10 − 10 M? A)

1.0 × 10− 7 M B) 1.0 × 10− 3 M C) 1.0 × 102 M D) 1.0 × 10− 4 M E) 1.0 × 10− 18 M

40)

Which of the following is incorrectly identified? A)

Ba(OH)2, strong base B) HF, strong acid C) NH3, weak base D) HCl, strong acid

41)

Calculate the acid concentration of a sample of acid rain with a pH of 8.11. A)

4.2 × 10-1 M B) 1.0 × 10-4 M C) 0.62 M D) 6.3 × 10-5 M E) 7.7 × 10-9 M

42)

What is the pOH of a solution with a pH of 11.5? A)

2.5 B) 0.115 C) 14.0 D) 0.25 E) 10.3

43)

What is the pH of a solution with [H3O+ ] = 1.0 × 10− 5 M? A)

9.0 B) 5.0 C) -9.0 D) -5.0 E) 1.0 × 10− 5

44) Which of the following is true in a acidic solution?A) [H+] = [OH−] B) [H+] > [OH−] C) [H+] < [OH−] D) [H+] = 0 E) [OH−] = 0

45) A solution with a pH of 8.0 is ___ times more basic than a solution with a pH of 6.0A) 1,000 B) 100 C) 10 D) 2 E) 0

46) The correct formula for hydrochloric acid is ___.A) HClO3 B) HCl C) HClO D) HClO2 E) H2Cl

47) The correct name for H2CO3 is ___ acid.A) carbonate B) carbonous C) hydrocarbonic D) carbonic E) hydrogen carbide

48) Calculate the unknown concentration of H3PO4 if 50.0mL was titrated to the end point with 16.50 mL of a

2.0 M NaOH solution according to the following acid-base titration.

H3PO4 (aq) + 3 NaOH(aq) → 2 H2O(l) + Na3PO4 (aq)

A) 0.22 M B) 0.033 M C) 0.011 M D) 11 M E) 3 M

49) What volume of 0.124 M KOH titrant was used to neutralize 23.4 mL of 0.206 M HCl solution?A) 15.9 mL B) 38.9 mL C) 31.8 mL D) 1.00 × 104 mL E) 5.00 × 102 mL

Chp. 13.1-13.2, 13.5Equilibrium / Le Châtelier’s Principle

For Questions 50 - 52, match the following to the energy diagram shown above.

50) activation energy, Ea 51) ΔHRXN 52) this reactions is A) A A) A A) exothermic

B) B B) B B) endothermicC) C C) C

Answer Questions 53 – 56 based on the equilibrium equation shown below.

CO2 (g) + H2(g) CO (g) + H2O(l) ΔHRXN = ─ 2.8 kJIn which direction will the equilibrium shift in response to each change listed below:

A)

towards productsB)

towards reactantsC)

no change

Chp. 11.1-11.8, 11.10Gas Laws

57)

Change Direction of Shift53) decrease temperature A) or B) or C)54) decrease volume A) or B) or C)55) add CO(g) A) or B) or C)56) remove some H2O(l) A) or B) or C)

The “initial volume” balloon is at atmospheric pressure. Which balloon(s) represent the “initial volume” balloon after it has been put into a chamber whose pressure is less than atmospheric?

A)

Balloon A B ) Balloon B C) Balloon C D) Balloons B and C E) Balloons A and B

58)

Complete the following statement: In Charles' law, the volume of a gas _____ when the _____ decreases.

A)

increases, quantity of gas B)

decreases, temperature C)

decreases, pressure D)

increases, pressure E)

increases, temperature

59)

What unit of temperature is used in gas law calculations? A)

Kelvin B)

Celsius C)

Fahrenheit D)

either Celsius or Fahrenheit E)

either Celsius or Kelvin

60)

In response to Boyle's law, the pressure of a gas increases as the volume decreases because A)

the gas particles strike the walls of the container more often. B)

the kinetic energy of the gas particles increases. C)

the gas particles get bigger. D)

the temperature of the gas increases. E)

the gas particles strike the walls of the container with more force.

61)

The boiling point of water at sea level is 100 °C. At higher altitudes, the boiling point of water will be A)

lower, because the atmospheric pressure is lower. B)

higher, because the altitude is greater. C)

the same, because water always boils at 100 °C. D)

higher, because there are fewer water molecules in the air. E)

lower, because temperatures are lower.

62)

The unit of 1 atmosphere used to describe the pressure of a gas is equal to ________. A)

1 mmHg B) 600 mmHg C) 200 mmHg D) 100 mmHg E) 760 mmHg

63)

The force of gas particles against the walls of a container is called ________. A)

volume b) density C) quantity of gas D) temperature E) pressure

64)

According to the kinetic molecular theory of gases, particles of a gas A)

are very large particles. B)

lose their valence electrons. C)

decrease in kinetic energy as temperature increases. D)

are very far apart. E)

move slowly.

65)

In Gay-Lussac's law, the pressure of a gas increases due to an increase in temperature because A)

there is a decrease in the volume of the container. B)

the molecules strike the walls of the container less often. C)

there is an increase in the number of gas particles. D)

the molecules strike the walls of the container harder and more often. E)

the molecules get bigger.

66)

According to Avogadro's law, the volume of a gas A)

depends only on the number of moles in the sample. B)

is directly related to the number of moles at constant temperature and pressure. C)

is inversely related to the number of moles at standard temperature and pressure. D)

is inversely related to the number of moles at constant temperature and pressure. E)

depends only on the temperature and pressure.

67)

At STP, temperature and pressure have the values of A)

0 K and 1 atm. B)

760 K and 273 atm. C)

0 K and 760 mmHg. D)

273 K and 1 mmHg. E)

273 K and 760 mmHg.

68)

In the kinetic molecular theory of gas behavior, the assumption is made that gas molecules A)

are attracted to each other by strong forces. B)

occasionally come to rest. C)

move with a kinetic energy equal to their centigrade temperature. D)

are close together in their container. E)

move rapidly in random directions.

69)

As you rise higher in Earth's atmosphere, the atmospheric pressure ________. A)

remains the same B) increases C) decreases

70) The mathematical expression of the ideal gas law is ________.

A) P1

T1 =

P2

T2

B) PV = nRT

C) P1V1 = P2V2

D) PT = P1 + P2 + P3….

E) V 1

P1 =

V 2

P2

71)

At STP, what is the volume of 1.0 mol of carbon dioxide? A)

1.00 L B) 12.2 L C) 273 L D) 22.4 L E) 44.0 L

72)

A kiloPascal is a unit of ________. A)

volume B) energy C) temperature D) mass E) pressure

73)

The pressure of 5.00 L of gas increases from 1.50 atm to 1.63 atm. What is the final volume of the gas, assuming constant temperature?

A)

5.00 L B) 4120 L C) 0.00600 L D) 4.60 L E) 5.40 L

74)

A 10.0 liter balloon was taken from a temperature of 298 K and placed in a freezer at a temperature of 258 K. What was the new volume if pressure is constant?

A)

8.66 liters B) 115 liters C) 2.50 liters D) 250. liters E) 11.60 L

75)

A gas contained in a steel tank has a pressure of 1.5 atm at a temperature of 320 K. What will be the gas pressure when the temperature changes to 450 K?

A)

2.1 atm B) 1.1 atm C) 0.47 atm D) 0.47 atm E) 0.94 atm

76)

At 570. mmHg and 298 K a gas sample has a volume of 2270 mL. What is the final pressure (in mmHg) at a volume of 1250 mL and a temperature of 448 K?

A)

7000 mmHg B) 690 mmHg C) 470 mmHg D) 210 mmHg E) 1560 mmHg

77)

The total pressure in a mixture of gases is equal to the partial pressure(s) of A)

the gas with the greatest number of moles. B)

all the gases added together. C)

the gas that occupies the largest volume. D)

the gas with the smallest number of moles. E)

the gas with the highest molecular weight.

78)

A cyclopropane-oxygen mixture is used as an anesthetic. If the partial pressure of cyclopropane in the mixture is 334 mmHg and the partial pressure of the oxygen is 1.02 atm, what is the total pressure of the mixture in torr?

A)

335 torr B) 432 torr C) 1.44 torr D) 1110 torr E) 760 torr

79)

A 0.315 mol sample of He gas has a pressure of 0.123 atm at 428 Kelvin. What is the volume of the sample?

A)

573 K B) 546 L C) 1.35 L D) 118 L E) 90.0 L

2013-14 GenChem Final ReviewPart II: FREE RESPONSE QUESTIONS:

For each mathematical question SHOW WORK, USE UNITS, and CIRCLE ANSWER

Refer to the equation shown below when answering Question 1.

2C2H2(g) + 5O2 → 4 CO2(g) + 2 H2O (g)Stoichiometry1. (a) What is the theoretical yield , in grams, of carbon dioxide if the reaction

starts with 5.0 g of hydrocarbon and excess oxygen?

(b) Calculate the percent yield if 15.0 g of CO2 are actually produced?

Acids and Bases2. Predict the products of the following neutralization reaction. Include phases of

matter. Balance the equation

H2SO4(aq) + Ba(OH)2(aq) →

Chemical Quantities3. Ascorbic acid (vitamin C), found in citrus fruits and vegetables, is important in metabolic reactions

160

in the body, in the synthesis of collagen, and to prevent scurvy. If ascorbic acid contains carbon (40.9%), hydrogen (4.58%), and oxygen (54.5%), what is the empirical formula of ascorbic acid?

Thermochemistry4. 5.0 g of CaCl2 is dissolved in 100. mL of distilled water in a coffee-cup calorimeter. The temperature increases from 21oC to 44.5oC.

(a) Is the dissolving of CaCl2 endothermic or exothermic? Justify your answer.

(b) Calculate the energy change, in kilojoules, caused by the dissolving of CaCl2. Assume the specific heat of the solution is

Acids and Bases161

5. A 2.0 M Ca(OH)2 solution is used to titrate a 30.0 mL sample of hydrochloric acid (HCl) of unknown concentration. The end point was reached after 12.35 mL of titrant had been added. The chemical equation representing this reaction is shown below.

2 HCl(aq) + Ca(OH)2(aq) → 2 H2O(l) + CaCl2(aq)

(a) Calculate the moles of titrant used.

(b) Calculate the moles of acid neutralized.

(c) Calculate the molarity of the HCl.

162

2013-14 GenChem Final ReviewEquations/ Constants/ Polyatomics / Solubility

Equations: Constantsq = mSHΔT

KW = [H3O+][OH−] KW = 1.0 x 10−14

14 = pH + pOH Avogadro's Number 6.022

x 1023

163

pH = − log [H3O+]

pOH = − log [OH−] R = 0.0821atm∙ Lmol ∙ K

M1V1 = M2V2

Molarity (M) = moles soluteliters solution SH H2O = 4.184 J

g •C o

V 1

T 1 = V 2

T 2

V1P1 = V2P2

PT = P1 + P2 + P3...

V 1P1

T 1 = V 2P2

T 2

PV = nRT

V 1

n1 = V 2

n2

P1

T1 = P2

T2

164

Solubility Rules

Soluble Compounds Insoluble Compounds

all ammonium (NH4+) compounds

all Group I compounds all nitrates (NO3

─) compounds all acetate (CH3COO─) compounds all chlorate (ClO3

─) compounds all perchlorates (ClO4

─) chlorides - except Ag+ Pb2+ , Hg2

2+

bromides - except Ag+ Pb2+ , Hg22+

iodides - except Ag+ Pb2+ , Hg22+

sulfates (SO42─) - except Ag+, Pb2+ , Ba2+, Sr2+, Ca2+

sulfides – except Ba2+, Ca2+, Sr2+

carbonates (CO32─)

phosphates (PO43─)

hydroxides (OH─) – except Ba2+, Ca2+, Sr2+

165

166