FTCE Chemistry SAE Preparation Course Session 1 Lisa Baig Instructor Deborah Derr Co-instructor.

FTCE Chemistry SAEPreparation Course

Session 1

Lisa BaigInstructor

Deborah DerrCo-instructor

Pre-Test

Pre-Test

• The answer key for the pre-test is now on the wiki

• You will receive a listing of competencies covered by each question, to better review the information you need further assistance in

http://subjectareatestprep.pds-hrd.wikispaces.net/Chemistry

Session Norms

• Respect– No side bars– Work on assigned materials only– Keep phones on vibrate– If a call must be taken, please leave the

room to do so

Chemistry Competencies

1. Knowledge of the nature of matter (11%)2. Knowledge of energy and its interaction with

matter (14%)3. Knowledge of bonding and molecular structure

(20%)4. Knowledge of chemical reactions and

stoichiometry (24%)5. Knowledge of atomic theory and structure (9%)6. Knowledge of the nature of science (13%)7. Knowledge of measurement (5%)8. Knowledge of appropriate laboratory use and

procedure (4%)

Course OutlineSession 1

Review Pre TestCompetencies 1 & 2

Session 2Competency 5



Session 5Competencies 6, 7 and 8

Post Test

Required Materials

• Scientific Calculator• Paper for notes• State Study Guide• SUGGESTED Book

– 5 Steps to a 5: AP Chemistry• Langley, Richard, & Moore, John. (2010). 5

steps to a 5: AP chemistry, 2010-2011 edition. New York, NY: McGraw Hill Professional.

Chemistry Competencies

1. Knowledge of the nature of matter (11%)2. Knowledge of energy and its interaction

with matter (14%)3. Knowledge of bonding and molecular structure (20%)4. Knowledge of chemical reactions and stoichiometry (24%)5. Knowledge of atomic theory and structure (9%)6. Knowledge of the nature of science (13%)7. Knowledge of measurement (5%)8. Knowledge of appropriate laboratory use and procedure

(4%)

Knowledge of theNature of Matter

Differentiate between pure substances, homogeneous mixtures and heterogeneous mixtures


Determine the effects of changes in temperature, volume, pressure or quantity

on an ideal gas

(Work with the various gas laws and their constants.)

P1V1=P2V2 P1 = P2 V1 = V2

T1 T2 T1 T2

P1V1 = P2V2 PV= nRT Values for R are given

T1 T2 on your reference sheet

Apply units of mass, volume and moles to determine concentrations and

dilutions of solutions.

Molarity (M) = moles/LiterMolality (m) = moles/kilogram

How many liters of solution are needed to make a 0.200M solution with 36.7g of

Calcium chloride?


How many liters of solution are needed to make a 0.200M solution with 36.7g of Calcium chloride?

Molarity = moles/Liter

36.7g CaCl2 =

110.984 g/mol=0.331 moles CaCl2

0.331 moles CaCl2 =

0.200 M solution= 1.65 L of solution

Analyze the effects of physical conditions on solubility and the

dissolving process

How do changes in the following affect solubility?

pressureheat

agitation


Evaluate problems relating colligative properties, molar mass and solution

processPactual = POXsolvent

If 18g of Sucrose (C12H22O11) are used in a 250mL cup of coffee. (80oC), What is the vapor pressure of the sugared coffee?


• How many moles of Sucrose? (C12H22O11) – Molar mass = 342 g/mol– Moles = 0.0526 mol

• 1 mL = 1g of water, so 250g of water – 13.89 mol H2O

13.89 mol H2O = X

13.89 mol H2O+ 0.0526 mol C12H22O11

X =.996• Vapor pressure of water at 80oC = 355.1

(reference sheet)• P = (355.1)(0.996)• P = 354 mmHg

• Analyze the effects of forces between chemical species on properties (eg, melting point, boiling point, vapor pressure, solubility, conductivity of matter)– ie- boiling point elevation, freezing point

depression

DT =kbm

DTt = -kf moles solute kg solvent


Practice problemWhat is the Freezing Point Depression if

2.84 moles of a solute are added to 0.687 kg of benzene?

Normal F.P = 5.48oCKf = 5.12 DTt = -kf moles solute

kg solventDTt = -5.12(2.84/.687)

DTt = -21.16

5.48oC -21.16oC=-15.68oC

• Solve problems involving an intensive property of matter– Density– Specific Heat

D = m/V Cp= . Q . m*DT


Practice problem

What is the energy absorbed by an 8.32g sample of Gold that goes from 37oC to 100oC? (Specific Heat of Gold = 0.129)

Cp= . Q . m*DT

0.129 = Q/(8.32•63)0.129•8.32•63=Q67.6J=Q

• Differentiate physical methods for separating the components of mixtures– Chromatography

• Combined liquids

– Extraction• Combined liquids

– Filtration• Solids within liquids


Break Time

Take a 10 minute

break!

Knowledge of Energy and its Interaction with Matter

• Distinguish between different forms of energy– Thermal– Electrical– Nuclear– Mechanical– Potential– Kinetic

The Kinetic Molecular Theory of Matter1) Gases consist of large numbers of tiny particles that

are far apart relative to their size2) Collisions between gas particles and between

particles and container walls are elastic collisions3) Gas particles are in continuous, rapid random

motion. They therefore possess kinetic energy, which is energy of motion

4) There are no forces of attraction between gas particles

5) The temperature of a gas depends on the average kinetic energy of the particles of the gas EK= ½ mv2


Phase Diagram

Temperature

Pressure

Points on Diagram

A = Triple PointB = Normal Melting Point

C = Normal Vaporization PointD = Critical Pressure Boiling Point

E = Critical Point

Wood, A. (2006, May). CO2 info. Retrieved from http://www.teamonslaught.fsnet.co.uk/co2_info.htm


As substance is heated, temperatures do NOT rise when it reaches a

melting/boiling point. Temperatures remain constant until all matter

reaches next state!

Calculate the enthalpy change for:C (s) + 2H2 (g) CH4 (g)

Given the following equations:Equation DHC + O2 CO2 -393.5

H2 + 1/2 O2 H2O -285.8

CH4 + 2 O2 CO2 + 2 H2O -890.3


We want C (s) + 2H2 (g) CH4 (g), so:

C + O2 CO2 -393.5

CO2 + 2 H2O CH4 + 2 O2 +890.3

2(H2 + ½ O2 H2O) 2(-285.8)

-74.8

• Predicting Entropy changes• Look at States of Matter

– Solids- LOW entropy– Liquids- Medium entropy– Gases- HIGH entropy

• Look at compounds-vs-elements– The more items in combination, the

more entropy



DH DS DG Spontaneous?

- + - Yes

- --

@ low temps

Yes@ low temps

+ +-

@ high temps

Yes@ high temps

+ - + No


DGo=DHo-TDSo

Temperature must be in KELVINS!!!DHo- • + = endothermic• - = exothermic


• Relate regions of the electromagnetic spectrum to the energy, wavelength and frequency of photons

E = h x vE = Energy of Quantum

h = 6.626 x 10-34 J•s (Planck’s Constant)v = frequency of the wave

C = l x vC = Speed of Light

3 x 108 m/s

l = wavelengthv= frequency

Homework

• A PDF file called “Session 1 Homework” is on the wiki

• Please access, and complete before session 2.

• We will review all the answers and procedures to answer at the start of session 2

FTCE Chemistry SAE Preparation Course Session 1 Lisa Baig Instructor Deborah Derr Co-instructor.

Documents

Transcript of FTCE Chemistry SAE Preparation Course Session 1 Lisa Baig Instructor Deborah Derr Co-instructor.