Chapter 11...The Mole
Define:
1. Mole:
2. Molar mass:
3. Empirical formula:
4. Molecular formula:
Fill in the following mole map:
Mass Moles Atoms/Molecules
Liters
Calculate the following:
5. How many moles of aluminum are in 162 grams of aluminum?
6. What is the molar mass of CaMg(CO3)2?
7. How many molecules of NaOH are in 112 liters of NaOH?
8. How many grams of N2 are present in 67.2 liters of N2?
9. How many molecules of Ca are present in 320 grams of Ca?
10. What is the percent composition of carbon in C6H12O6?
11. How many moles of oxygen are in three moles of Mg(NO3)2?
Determine the empirical formula for the following:
12. 22.1% aluminum, 25.4% phosphorus, 52.5% oxygen:
Determine the molecular formula for the following:
13. What is the molecular formula of a compound that has 40.00% carbon, 6.67% hydrogen and 53.33% oxygen, and has a molar mass of 150 amu’s?
Chapter 12…Stoichiometry
Use the following reaction to answer the questions that follow:
Fe(s) + O2 (g) Fe2O3 (s)
1. How many grams of Fe2O3 will be produced from 213 grams of Fe?
2. How many liters of O2 are required to produce 96 grams of Fe2O3?
Fe(s) + O2 (g) Fe2O3 (s)
3. How many grams of iron are required to react with 82 liters of O2?
4. In the following reaction: H2 (g) + N2(g) NH3 (g) How many liters of H2 are required to
produce 16.8 liters of NH3?
5. A sample of 23.4 grams of sodium hydroxide is mixed with 18.7 grams of lithium sulfide, producing lithium hydroxide and sodium sulfide. What is the limiting reagent? How many grams of lithium hydroxide are produced?
6. LiOH + KCl à LiCl + KOH
a) I began this reaction with 20 grams of lithium hydroxide. What is my theoretical yield of lithium chloride?
b) I actually produced 6 grams of lithium chloride. What is my percent yield?
Chapter 13…States of Matter
Define:
1. Vapor Pressure:
2. Freezing Point:
3. Melting Point:
4. Boiling Point:
5. Condensation Point:
6. Sublimation:
8. Triple Point:
5. Tyndall Effect:
Use the Phase Diagram Below to Answer the Following Questions:
1. What is the triple point of the substance depicted in the phase diagram above?
2. What is the melting point? ______freezing point? ______
3. What phase is this substance in at –67°C and 3900 mm Hg of pressure?
Chapter 14…Kinetic Theory
Define:
1. Barometer:
2. Temperature:
3. Gas Pressure:
4. Kinetic Energy:
5. Heat:
6. Absolute Zero:
Short Answer:
7. Relationship between volume and # of collisions:
8. Relationship between temperature and # of collisions:
9. Relationship between pressure and # of collisions:
10. Relationship between volume and pressure:
11. Relationship between temperature and volume:
12. Heat always flows from ______to ______.
Temperature Conversions:
12. 334 K = ______°C 13. 25°C = ______K
Pressure Conversions:
14. 0.96 atm = ______kPa 15. 324 kPa = ______mmHg 16. 956 mmHg = ______atm
Chapter 14 cont...Gas Laws
Write the equations for the following and indicate what is held constant:
1. Boyle’s Law:
2. Charles’ Law:
3. Gay-Lussac’s Law:
4. Combined Gas Law:
5. Ideal Gas Law:
6. Density:
7. Indicate the relationship between the variables in each of the equations above.
8. Indicate what each variable stands for in each of the equations above.
9. Temperature is in what unit for gas laws?
10. STP stands for:
11. Standard temperature = ______
12. Standard pressure = ______atm, ______kPa or ______mmHg
13. What is the relationship between: volume and density:
temperature and density:
pressure and density
Calculate the following:
14. A sample of argon gas is cooled and its volume went from 830 mL to 520 mL. If its final temperature was
35°C, what was its original temperature?
15. A sealed container of nitrogen gas has a pressure of 780 kPa and a temperature of 18°C. The can of gas is
left in a hot car and the temperature of the gas increases to 65°C. What is the new pressure in the can?
16. A sample of fluorine gas exerts a pressure of 900 mmHg. When the pressure is changed to 1.75 atm, it
occupies 500 mL. What was the original volume of the gas in liters?
17. How many moles of O2 gas will occupy a volume of 435 mL at 267 kPa and 25°C? How many molecules
of O2?
18. A 300 mL sample of CO2 is submitted to conditions of 5.2 atm and 33°C. What would the volume of this
gas be at STP?
Chapter 15…Solutions
Define:
1. Solution:
2. Solute:
3. Solvent:
4. Miscible:
5. Dilute
6. Concentrated:
7. Saturated solution:
8. Unsaturated solution:
9. Supersaturated solution:
10. Precipitate:
Use the solubility graph below to answer questions 11-14:
11. How many grams of NaNO3 will dissolve at 30°C?
12. Which substance is least soluble at 10°C?
13. Which two substances have the same solubility at 72°C?
14. 80 grams of KBr placed in 60°C creates a (saturated/unsaturated/supersaturated) solution.
15. When Be(NO3)2 (aq) and NaOH (aq) are mixed together, the resulting precipitate is:
16. Placing a solute in a solvent will (increase/decrease) the boiling point and (increase/decrease) the freezing
point of a solution.
17. (Ionic/molecular) compounds cause greater change of boiling/freezing points in solutions.
18. Aluminum chloride (AlCl3) will dissociate into _____(how many) ions and will cause a (greater/smaller)
change boiling point than MgCl2.
19. In the solvation of solids, solubility rate increases with (high/low) temperatures and (high /low) pressure.
20. In the solvation of gases, solubility rate increases with (high/low) temperatures and (high /low) pressure.
21. The general rule for solvation is “______dissolves ______”.
For each of the following reactions…
a) Finish and balance the chemical reaction
b) Use a solubility chart to predict what precipitate will form in the reaction
c) Write the complete ionic equation
d) Write the net ionic equation
22.) Al(ClO4)3 (aq) + K2CO3 (aq)
a)
b)
c)
d)
23.) AgNO3 (aq) + H2S (aq)
a)
b)
c)
d)
Compound / Solubility / ExceptionsSalts of group 1A and ammonia (NH3) / Soluble (aq) / Some lithium compounds
Ethanoates, nitrates, chlorates, and perchlorates / Soluble (aq) / Few Exceptions
Sulfates (SO4) / Soluble (aq) / Compounds of Pb, Ag, Hg, Ba, Sr, and Ca
Chlorides, Bromides, and Iodides / Soluble (aq) / Compounds of Ag and some of Hg and Pb
Sulfides and Hydroxides / Insoluble (s) / Group 1A compounds. Compounds of Ba, Sr, and Ca (slightly)
Carbonates, Phosphates, and Sulfites / Insoluble (s) / Group 1A and ammonia (NH3) compounds
Chapter 16…Thermodynamics
Define and give the symbols (if any) for the following:
1. Entropy:
2. Enthalpy:
3. In general, spontaneous reactions favor (endothermic/exothermic) reactions and a(n) (decrease/increase) in
entropy.
4. Rank the four states of matter (gas, liquid, plasma, solid) in order of decreasing entropy:
5. In the reaction: NH3 (g) + HCl (g) NH4Cl (s) entropy (decreases/increases).
6. Standard conditions in thermodynamics are: ______°C, ______K, ______atm, ______kPa and
______mmHg.
Label the Following Lines on the Heating Curve as: Boiling Pt., Melting Pt., Liquid, Vapor or Gas:
4. Calculate the amount of energy required to heat a 150 g chunk of aluminum from 20°C to 40°C. (Cp of aluminum = 0.220 cal/g°C)
Chapters 17& 18…Reaction Rates & Equilibrium
Define:
1. Equilibrium:
2. Activated complex:
3. Activation energy:
4. Catalyst:
5. Inhibitor:
7. The reaction rate expression for an irreversible reaction is: Rate = ______
8. The equilibrium constant expression for a reversible reaction is Keq = ______
10. List the six factors that can affect the rate of reaction:
a. b. c.
d. e. f.
Use the equation below to answer the following questions:
H2 (g) + Br2 (g) 2 HBr (g) + Heat
11. Write the rate expression for this reversible reaction at equilibrium:
12. What is Keq if the concentrations of H2 and Br2 are each 2.0 M, and the concentrations of HBr is 3.0 M?
13. Do more products or reactants exist at equilibrium?
14. If more H2 is added to this reaction, equilibrium will shift (left/right/no shift).
15. If Br2 is removed from this reaction, equilibrium will shift (left/right/no shift).
16. If pressure is increased, equilibrium will shift (left/right/no shift).
17. If temperature is decreased, equilibrium will shift (left/right/no shift).
18. If HBr is increased, equilibrium will shift (left/right/no shift).
20. A catalyst (does/does not) become part of a chemical reaction.
55) According to the Common Ion effect, what will happen at equilibrium to the equation: BaSO4(s) + Na2SO4(aq) →
56) List the 3 reasons some rxns are not reversible.
Chapter 19…Acids, Bases and Salts
1. Acid
2. Base:
3. Salt:
4. Amphoteric:
5. Polyprotic acid:
6. Binary acid:
7. Ternary acid:
8. Acidic anhydride:
9. Basic anhydride:
10. Electrolyte:
Fill in the following table of acid-base theories:
Acids / BasesArrhenius Theory
Bronsted-Lowry Theory
Lewis Theory
Name the following: Write the formulas for the following:
15. HC2H3O2: 18. hydrosulfuric acid:
16. HF: 19. perchloric acid:
17. H2SO3: 20. nitrous acid:
21. Label the compounds in the following reaction as conjugate acid (CA), conjugate base (CB), acid and base:
OH (aq) + H2CO3 (aq) HCO3 (aq) + H2O (l)
22. Write the Ka expression for the above equation:
23. Water ionizes into ______and ______.
24. The value for Kw is always equal to ______.
25. If the concentration OH- is 6.3 x 10-3, what is the concentration of H3O+ in water?
26. Is the above solution acidic or basic?
27. What are the products of a neutralization reaction?
Use the following concentration to answer questions 26-29:
**[H+] concentration of 3.62 x 10-12
28. pH =
29. pOH =
30. [OH-] concentration =
31. Is this solution acidic or basic?
Chapter 22...Organic- Hydrocarbons
Define:
1. Hydrocarbon:
2. Alkane:
3. Alkene:
4. Alkyne:
5. Functional group:
Identify the following prefixes:
12. one carbon: 16. five carbons: 19. eight carbons:
13. two carbons: 17. six carbons: 20. nine carbons:
14. three carbons: 18. seven carbons: 21. ten carbons:
15. four carbons:
Identify the following as an Name the following:
alkane, alkene, or alkyne: 25. Alkyne with 9 carbons:
22. C3H6:
23. C6H10: 26.
24. C2H6:
Identify the following
functional groups:
29. R–OH: 27. C8H18:
30. R-O-R:
31. R-NH2 28.
31. R-CHO or
32. R-CO-R or
33. R-COOH or
34. R-COO-R or
8