Final Exam Review Packet s1

Honors Chemistry

FINAL EXAM REVIEW PACKET

Spring Semester 2015

The format of the final exam is MULTIPLE CHOICE. This review packet is intended to inform you of the content in each unit covered and allow you practice with the content from this semester. It is not intended to address any specific test question on the final exam. Completion of this packet does not guarantee success on the Final Exam, but practicing with the content is a great idea. Unit 11: Stoichiometry and Limiting Reactants Ch. 11 Mole ratios, mass-mass/volume-volume/moles-mass problems, percent yield, Limiting Reactants

DEFINE:

a. mole ratio

b. stoichiometry

c. percent yield

d. theoretical yield

e. actual yield

f. limiting reactant

g. excess reactant

h. Law of Conservation of Mass

1. Answer the following questions about stoichiometry problems:

a. Where do the numbers for a mole ratio come from?

b. Why is a mole ratio important in a stoichiometry problem?

c. When would you know to use the Avogadro number as a conversion factor in a stoichiometry problem?

2. Calculate the mass of silver phosphate produced if 30.0 g of silver acetate reacts with excess sodium phosphate.

AgC2H3O2 + Na3PO4 (aq) → Ag3PO4 + NaC2H3O2

3. Aspirin can be made from salicylic acid and acetic anhydride. Suppose you mix 13.2 grams of salicylic acid with 50.9 grams of acetic anhydride and obtain 5.9 grams of aspirin and some water in the lab. Calculate the percent yield of aspirin. Unit 12: Thermochemistry Ch. 15 Energy, specific heat, enthalpy, joules, calorimetry

DEFINE:

a. Exothermic

b. Endothermic

c. Activation Energy

d. Calorie

1. A silver bar with a mass of 250.0 g is heated from 22.0°C to 68.5°C. How much heat does the silver bar absorb?

2. A 15.6 g sample of ethanol absorbs 868 J as it is heated. If the initial temperature of the ethanol was 21.5°C, what is the final temperature of the ethanol?

3. How much heat is released when 82.1 g of methanol is burned according to the following equation?

CH3OH(l) + 3O2 (g) → 2CO2(g) + 3H2O (l) ∆H = -726 kJ/mol

4. What mass of benzene must be burned in order to liberate 1.00 x 104 kJ of heat?

2C6H6 (l) + 15O2 (g) → 12CO2(g) + 6H2O (l) ∆H = -3268 kJ/mol

Unit 13: States of Matter Ch. 12 Solids, liquids, phase changes, intermolecular forces, phase diagrams

DEFINE:

a. Intermolecular forces (IMF) b. Triple point

c. Critical point

d. Hydrogen Bonding

e. London Dispersion Forces

1. Dispersion forces, dipole-dipole forces, and hydrogen bonds are examples of what type of forces? Describe dispersion forces.

2. Dispersion forces are greatest between what type of molecules?

3. Describe dipole-dipole forces.

4. Describe a hydrogen bond.

5. Identify each of the diagrams below as illustrating dipole-dipole forces, dispersion forces, or hydrogen bonds.

6. Rank dipole-dipole forces, dispersion forces, and hydrogen bonds in order of increasing strength.

Use the phase diagram for water to answer the following questions.

10. What does point 1 represent?

11. What is point 4 called? What does it represent? Unit 14: Gas Laws Ch. 12 (sect 1 only), 13 Pressure, Molar volume, Boyle’s/Charles’/Gay-Lussac/Combined/Ideal Gas Laws, Dalton’s Law of Partial Pressure

DEFINE:

a. Boyle’s Law

b. Charle’s Law

c. Gay-Lussac’s Law

d. Combined Gas Law

e. Ideal Gas Law

f. Dalton’s Law

g. STP

h. Kinetic Molecular Theory

Use each of the terms below to complete the passage. Each term may be used more than once.

pressure temperature volume

Boyle's law relates (9) ______and (10) ______if (11) ______and amount of gas are held constant. Charles's law relates (12) ______and

(13) ______if (14) ______and amount of gas are held constant. Gay-Lussac's law relates (15) ______and (16) ______if (17) ______and amount of gas are held constant. Match the definition in Column A with the term in Column B.

Column A Column B ______20. Equal volumes of gases at the same temperature and pressure a. Avogadro's contain equal numbers of particles. principle

______21. One mole of any gas will occupy a volume of 22.4 L at STP. b. Boyle's law

______22. R represents the relationship among pressure, volume, temperature, c. Charles's law and number of moles of gas present. d. combined gas law ______23. Temperature, pressure, and volume are related for a fixed amount of gas. e. Gay-Lussac's law

______24. The physical behavior of an ideal gas can be expressed in terms of f. ideal gas the pressure, volume, temperature, and number of moles of gas constant present. g. ideal gas law ______25. The pressure of a given mass of gas varies directly with the kelvin temperature when the volume remains constant. h. molar volume

______26. The volume of a given amount of gas held at a constant temperature varies inversely with the pressure.

______27. The volume of a given mass of gas is directly proportional to its kelvin temperature at constant pressure

28. Solve for the missing variable using the appropriate gas law(s) for the conditions given:

a. V1= 1.028 L, P1= 0.99 atm, P2= 110.2 kPa, V2= ? d. V1= 550 mL, P1= 766 torr, P2=?, V2= 2.60 L

o 3 o o b. V1= 1.028 L, T1= 99 C, V2= 4.102 L, T2= ? e. V1= 1556 cm , T1= 59 C, V2= ?, T2= 17 C

o o c. T1= 102.8 C, P1= 0.99 atm, P2= 810.2 mmHg, T2= ? f. T1= 12.8 C, P1= 2.5 atm, P2= ? T2= 300 K 29. Calculate the volume of a gas at STP given the following conditions:

o a. V1= 1.028 L, P1= 0.99 atm, T1= 99 C

o b. V1= 546 mL, P1= 550 mmHg, T1= 9.9 C

3 o c. V1= 2.4 dm , P1= 110.2 kPa, T1= 211 C

3 o d. V1= 2448 cm , P1= 689.5 torr, T1= 15.60 C

30. Solve for the missing variable using the appropriate gas law(s) for the conditions given:

a. V=?, P=699 mmHg, T= 78.5 oC, n=0.56 moles

b. n=?, V=1234 mL, P=1.25 atm, T=0 oC

c. P=?, T=25.0 oC, V= 22.4 L, n=3.2 moles

d. T=?, P=760 torr, V=22.4 L, n=1.00 moles

31. What is the partial pressure of oxygen gas in a mixture of nitrogen gas and oxygen gas with a total pressure of 0.48 atm if the partial pressure of nitrogen gas is 0.24 atm?

32. Use Graham’s Law of Effusion to solve the following: a. Calculate the ratio of diffusion rates for neon and helium. Which diffuses faster? About how much fatser? b. Calculate the ratio of diffusion rates for ammonia and carbon dioxide. Which diffuses more rapidly?

-6 c. Tetrafluoroethlene (C2F4) effuses at a rate of 4.6 x 10 moles/hr. An unknown gas effuses at a rate of 6.5 x 10-6 moles/hr under identical conditions. What is the molar mass of the unknown gas?

Unit 15: Solutions Ch. 14 Solute, Solvent, Concentration, Factors affecting Solvation, Colligative Properties

DEFINE:

a. solute

b. solvent

c. alloy

d. molarity

e. molality

Use each of the terms below just once to complete the passage.

immiscible liquid soluble solution insoluble miscible solute solvent Air is a(n) (1) ______of oxygen gas dissolved in nitrogen gas. The oxygen in air is the (2)

______, and nitrogen is the (3) ______. Because oxygen gas dissolves in a solvent, oxygen gas is a(n) (4) ______substance. A substance that does not dissolve is

(5) ______. (6) ______solutions are the most common type of solutions. If one liquid is soluble in another liquid, such as acetic acid in water, the two liquids are (7) ______.

However, if one liquid is insoluble in another, the liquids are (8) ______.

Use the following graph to answer these questions.

1. The y axis measures the amount of solute that will dissolve into a given amount of solvent. Identify the solvent in the solutions represented by the graph, and describe how much of it will be used to create the solution. 2. The x axis describes the conditions under which the solution has been created. Based on this graph, what factor affects the amount of solute that can dissolve? What other unit(s) might this variable be measured in?

3. At which temperature do KBr and KNO3 have the same solubility?

o 4. At 60 C, how much KNO3 can 100 g of water hold? 5. Which compound's solubility changes very little with temperature? 6. Which compound's solubility changes the most with temperature? 7. Which compound has the greatest solubility at 60oC? 8. Which compound has the least solubility at 20o C?

9. The substances listed on the graph are either solids or liquids. How would the solubility curve of a gas be different? Why would it be different?

Unit 16: Equilibrium Ch. 17 (sect. 1-3 only) Equilibrium, LeChatelier’s Principle, catalysts

DEFINE:

a. reversible reaction

b. equilibrium

c. catalyst

d. LeChatlier’s Principle

1. Explain why the amounts of the products and reactants present in a chemical reaction are not always equal when the system is at equilibrium.

2. Assume for the equilibrium

PCl5 (g) → PCl3 (g) + Cl2 (g) ΔH = 92.9 kJ

A. What is the effect on Kc of lowering the temperature?

B. What is the effect on the equilibrium concentration of PCl5 of adding Cl2?

C. What is the effect on the equilibrium concentrations of compressing the mixture to a smaller volume?

D. What is the effect on the equilibrium pressure of Cl2 of removing PCl3?

Unit 17: Acids and Bases Ch. 18

Arrhenius/Bronsted-Lowry Models, pH, pOH, Ka, Kb, auto ionization of H2O, neutralization, buffers

DEFINE: a. Arrhenius acid

b. Arrhenius base

c. Bronsted-Lowry acid

d. Bronsted-Lowry base

e. Hydronium ion

f. Hydroxide ion

g. Salt

h. Neutralization reaction

j. pOH

k. indicator

l. titration

m. strong acid

n. strong base

o. weak acid

p. weak base

1. Name three properties of acids and bases

2. Name or write the formulas for the following acids.

nitrous acid H2S

hydrochloric acid HNO3

carbonic acid H3PO2

sulfuric acid HClO4

hydroiodic acid HC2H3O2 hypobromous acid HF

sulfurous acid H2C2O4

chloric acid H2SeO4

hyponitrous acid HI

iodic acid H3P

3. What is the pH of the following solutions:

-9 a) 4.2 x 10 M HCl

-1 b) 1 x 10 M Ba(OH)2

-7 c) 6.7 x 10 M H3PO4

-4 d) 7.6 x 10 M Al(OH)3

Unit 18: Oxidation Reduction Reactions (Redox) Ch. 19 & 20

Oxidation numbers, balancing redox, Ecell, Batteries

DEFINE:

a. oxidation

b. reduction

c. oxidizing agent

d. reducing agent

e. OIL RIG

f. LEO GER

g. Half-reaction method

h. battery