Final Review
Academic Chemistry Second Semester 2016
Chapter 7- Chemical Reactions
Chapter 9- Chemical Quantities Chapter 10 Heat Energy
Chapter 13- Gas Laws
Chapter 15 solutions
Chapter 17-Kinetics
You must complete the 12 required questions on the answer sheet!
SECTION A
Chapter 6 and 9 Moles and Stoichiometry
Be able to:
Convert to and from moles, grams, liters, and particles.
Know constants equal to 1 mole
Know what STP is for 1 mole of any gas
 Find % composition of a formula
Find empirical formula using mole ratios
Find the unknown in moles, grams, liter, and particles given a known amount from a balanced equation.
Identify and use the limiting reactant to find an unknown of either a product or reactant.
Solve for formula of a hydrate with given data.
Solve for moles of a product with given data.
Solve for % yield
Identify the difference between actual and theoretical yield.
Find the theoretical yield of an unknown from any given from the balanced reaction.
Be able to change chemical A to chemical B from a balanced chemical equation and using any of these: mass,
molecules, atoms, liters. (Stoichiometry)
1 Solve for unknown.
a. Change 5.0 moles of Ag to mass
b. What is the molar mass of barium nitrate?
c. How many grams of NH3 are in 44.8 L of this gas at STP?
d. Change 25.6 g of perchloric acid to molecules.
e. Sulfur atoms in 96.3 g of sulfur is
2. Determine the empirical formula for a compound with 80.0 g of C and 20.0 g of H
3.Determine the empirical formula and name of the compound made when 8.65 g of iron combines with 3.72 g of
oxygen.
4. A student’s experiment was expected to produce 2.44 g of NaCl. When they weighed the product after the reaction,
only 2.23 g of NaCl was present. The percent yield was:
5. What is the mass of the metal present in 20 g of chromium II chloride?
6.The maximum of a product that can be formed given the amounts of reactants used is called ________________
And the maximum amount of product is determined by the _________________________________
7. Find the empirical formula that contains 1.44 g Mg and .948 g of O. Name this compound
8. Zn + 2 HCl  ZnCl2 + H2 If 4.13 moles of HCl are used, how many moles of ZnCl2 are produced?
9. Mg3N2(aq) +H2O(l)
Mg(OH)2(Aq) + NH3(g) If the initial amount of Mg3N2 is 7.70 g and the initial amount of H2O
is 10.22, what volume of ammonia gas can be produced? What is the limiting reactant? (Balance equation, then
solve for both givens. The smallest is the amount produced.)
10. The average human requires 120.0 grams of glucose (C6H12O6) per day. How many grams of CO2are required for this
amount of glucose? C6H12O6 + O2  CO2 + H2O (Balance equation, then solve for grams of CO2)
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11. AgNO3(aq) + Na2SO4(aq)  Ag2SO4(s) + NaNO3(aq) How many grams of silver sulfate (Ag2SO4)can be
produced from the reaction of 17.0g of silver nitrate (AgNO3) with 34.0g sodium sulfate solution? (Balance equation,
then solve for both givens. The smallest is the amount produced.)
12. How many grams of calcium chloride are required to completely react with 21.0 g of sodium phosphate?
3CaCl2 + 2Na3PO4  Ca3(PO4)2 + 6NaCl
13. What is the % phosphate in phosphoric acid?
A chemical reaction was the result of combining sodium hydrogen carbonate with hydrochloric acid. #14-16. The data was collected
before and after the reaction with sodium hydrogen carbonate and hydrochloric acid. The reactants were heated until no liquid
remained. The products of the reaction included water as a vapor and a gas in addition to the salt left in the evaporating dish.
DATA TABLE NaHCO3 + HCl  NaCl + H2O + CO2
Mass of empty crucible
22.63
Mass of sodium hydrogen carbonate
Molar mass = 84.00684
Before reaction Mass of crucible 25.76
After heat and reaction Mass of crucible 24.74
+ sodium hydrogen carbonate
+ salt
Molar mass = 58.442768
14.How many moles of salt were recovered in this experiment?
15. Using the actual yield of salt from the data and calculating the theoretical yield from the mass of the reactant,
what is the % yield of the salt?
16.If 2.00 grams of salt are recovered what should be the actual amount of carbon dioxide in grams?
17. Given the following reaction: 2H2 + O2  2H2O . How many water molecules are produced if 2.3 mol of oxygen
reacts with excess hydrogen?
18. How many grams of carbon dioxide are produced when 100 g of propane, C3H8 are combusted?
C3H8 + 5O2  3CO2 + 4H2O
19. How many grams of H3PO4 are produced when 5.99 x 1024 molecules of water react with 235.0 g of P4O10?
P4O10 + 6 H2O  3H3PO4
SECTION B
CHAPTER 13 GAS LAWS
Be able to:
Identify the properties and characteristics of gases.
 Use STP values in gas law problems
Convert units of pressure to and from atm, kPa, and mmHg.
Convert units of temperature to and from C and K.
Use and apply gas law formulas for Boyle’s, Charles’, Guy-Lusaac, Combined, and Ideal laws.
Recognize everyday examples of gas laws.
Know why a He balloon shrinks in cold and expand in warm.
1. Use this equation to answer questions 1-3. 2C8H18 + 25O2  16CO2 + 18H2O
Octane is combusted in a gasoline engine and produces water vapor and carbon dioxide gas.
How many liters of carbon dioxide gas are produced at 1.05 atm and a temperature of 212 C when 150 g of octane are
burned? (Change g of C8H18 to moles of CO2 using stoichiometry. Change moles of CO2 to volume of CO2 using the ideal gas
law.)
2. When 230 g of octane combust in the presence of oxygen at a volume of 980.0 L and a temperature of 199 C, what is the pressure
of oxygen? (Change grams of octane to moles of O 2 using stoichiometry. Change moles of O2 to pressure using ideal gas law.)
3. If 100.00 liters of water vapor is produced at a temperature of 236 ºC and a pressure of 1.10 atm, how many grams of octane
reacted? (Change volume of water to moles of water using the ideal gas law. Change moles of water to grams of C 8H18 using
stoichiometry.)
4. A gas occupies 19.53L at 0.899 atm at 212 C. What will be the volume of this gas if the pressure becomes 3.00 atm at a
temperature of 312 C?
5. If the initial pressure and temperature of gas is at STP, and the temperature is raised to 10.67 C, what is the new
pressure in mm Hg?
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6. A gas occupies a volume of 30 mL at 273 K. If the temperature is increased to 364 K while the pressure remains
constant, what will be the volume of the gas?
7. What is the resulting volume when 0.825 liter of a gas is cooled from 50.0 oC to 20.0oC and subjected to a
pressure change from 1.45 atm to 1.00 atm?
8. How many moles of O2 must be placed in a rigid container whose volume is 50.0 L in order to produce a
pressure of 4.50 atm at 273K?
9. Identify the gas law and explanation for the results of the following demonstrations.
10. What mass of potassium chlorate was decomposed if 62.50 L of O2 gas was collected at 210.0 C and 856.0 mmHg?
(change liters of O2 to moles of O2 with ideal gas law. change moles of O2 to mass of KClO3 using stoichiometry.)
Vacuum pump with balloon
Vacuum pump with boil water
Vacuum pump shave cream
Straw
Can crush
Balloon inside bottle
Balloons in hot and cold
Balloons on bottles in hot/cold
Air freshener
Baggie in beaker
Hand boiler
Can of air
SECTION C
CHAPTER 10 ENERGY
Be able to:
Identify phase changes on a heating curve.
 Identify where water is a solid, liquid and gas on a heating curve.
Solve specific heat problems.
Solve ∆H problems.
Recognize endothermic and exothermic systems.
Recognize how increasing or decreasing the heat energy changes the motion and energy of the particle.
Know why a He balloon shrinks in cold and expand in warm.
1.What is The law of conservation of energy ?
2. How much heat is given off when 124.0 g of methane (CH 4) is burned with oxygen, as shown in the
following thermochemical equation? CH4 + 2O2  CO2 + 2H2O + 890 kJ
3. When CaCl2 dissolves in 225.0g of water in a calorimeter, the temperature of the water increases by 2.95°C.
How much heat energy has been gained by the water? Assume that all the heat is absorbed by the water
(c=4.18J/g°C)
4. What is the specific heat of 63.95 g of metal which transfers 249.50J of heat with a final
temperature of 23.60°C and an initial temperature of 20.30°C?
5. Define
a. Specific heat
b. Exothermic
c. Endothermic
d. Heat of fusion
e. Heat of
vaporization
f. Temperature
g. Heat
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HEAT
6.
18 g or ice at -11° C are changed to steam at 125°C, how much Energy in J is required. Show all work.
1.
2.
3.
4.
5.
6.
7. Calculate the heat energy when 100 g of wax are burned.
C25H52 + 38O2  25CO2 + 26H2O +14600 kJ
SECTION D
Ch 15 solutions
Be able to :
Recognize M for molarity of a solution.
Solve for the molarity of a solution.
Identify the factors which affect the rate of dissolving of a substance.
Know the definitions for : Saturated, Unsaturated, Solubility, Insoluble , Colligative property, freezing point
depression, boiling point elevation
Identify the solute and solvent in a solution.
Calculate % concentration by mass or volume
Calculate new concentration or volume in a dilution problem.
1. What is the number of moles of solute in 10.5 L of a 0.250 M solution?
2. 10.0 grams of sugar is dissolved in 100.0 mL of water. The solvent is:
3.What is the molarity of a solution containing 9.0 moles of solute in 500.0 mL of solution?
4. How many liters of solution are present if the molarity is 2.75 M and there are 4.63 moles of solute dissolved?
5.What is the number of moles dissolved in a solution with a molarity of 0.550M with a volume of 600.0 L?
6. Define each term
A.Saturated
B.Unsaturated
C.
Solubility
D. Insoluble
E.Colligative
property
7. What is the new concentration of a solution that begins with a concentration of 0.25M and a volume of 3.50 L
and the new volume is 5.0 L?
Note: The next page is the answer sheet for the required questions. Make sure to print it on 1 sheet only.
DUE NO LATER THAN YOUR CLASS PERIOD ON WED, 5/18!!
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Name ____________________________________________________ SEMESTER II EXAM STUDY GUIDE -----/30
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