QUATERLY 3 REVIEW
CHAPTER 12- Stoichiometry
1. Define the law of conservation of mass
2. Calculate the mass of a product when given the mass / moles of reactant(s)
3. Define Limiting and excess reagent
4. Determine the limiting and excess reagents from given data
5. Define Percent Yield and calculate it from given data
6. a. What mass of iron must react with excess oxygen in order to form 4.81 moles of iron (III) oxide? b. What mass of iron is needed to
react with 40.0 g of oxygen?
7. Predict the mass of barium phosphate that will be formed if 20.2g of barium nitrate reacts with 18.0g of sodium phosphate. Which
substance is limiting reactant? How much of excess is left over? If in the lab 12.3 g of barium phosphate were produced, what’s the
percent yield?
Chapter 13 – Solids and Liquids
Identify all types of intermolecular forces in 1-4:
1. Attraction between any two polar molecules.
2. Very weak force that increases with molar mass.
3. Attraction between two induced dipoles.
4. Very strong attractive force between molecules with N-H,
O-H, or F-H bonds.
5. Compare and contrast solids and liquids.
Identify the type of solid in 6-10:
6. Every atom is covalently bonded to another atom.
7. Atoms are surrounded by a sea of electrons.
8. Particles are connected only by IMF
9. There is no geometric pattern in the structure.
10. Charged particles in a geometric pattern
Chapter 14 – Gases
13. A jar is tightly sealed at 22°C and 772 mmHg. What is the
pressure inside the jar after it has been heated to 178°C?
14. 300.0 mL of gas has a pressure of 75.0 kPa. When the
volume is decreased to 125.0 mL, what is its pressure?
15. 50.0 L of gas has a temperature of 75°C. What is the temp
in Celsius when the volume changes to 110. L?
16. What is the volume of a container that holds 48.0 g of
helium at a pressure of 4.0 atm and temperature of 52°C?
17. A gas occupies 325 L at 25°C and 98.0 kPa. What is its
volume at 70.0 kPa and 15°C?
Chapter 15 – Solutions
21. Explain the effect of adding more solute to unsaturated,
saturated and supersaturated solutions.
22. Explain how temperature and pressure affect solubility.
State whether each pair is soluble or insoluble in 23-26.
23. KCl in water
25. Wax in gasoline
24. Ammonia in oil
26. Methane in water
27. Use solubility table to answer:
a. How much KClO3 is dissolved in 200 g of water at
60°C?
b. What mass of additional CaCl2 is dissolved in 50 g of
water if the temp. rises from 10°C to 20°C?
c. How would the slope of the KClO3 line differ from CO2
28. How many grams of AlCl3 are required to make a 2.25m
solution in 30.0 g of water?
29. What volume of 12M HCl is needed to prepare 250 mL of
0.20M HCl?
30. Explain the difference in preparing solutions based on
molarity vs. molality.
31. Which will have the greatest effect on Tf at the same
molality: C12H22O11, MgBr2, AlCl3, or NH4NO3?
32. When 26.4 g of NaBr dissolves in 0.20 kg of water, what is
the freezing point and boiling point of the solution?(Kf=
1.86°C/m and Kb=0.512°C/m)
11. Explain the relationship between strong intermolecular
forces and the following properties – volatility, vapor
pressure and boiling point.
12. Hydrogen diffuses 3.72 times faster than an unknown gas.
Find the molar mass of the unknown gas.
VOCAB: surface tension
crystalline vs. amorphous
capillary action
sublimation
volatility
diffusion
vapor pressure
effusion
boiling point
Dalton’s Law of PP
hydrogen bond
London-dispersion forces
dipole-dipole forces
viscosity
phase diagram
18. What is the molar mass of an unknown gas if a sample has
a mass of 0.290 g and occupies a volume of 148 mL at 13°C
and a pressure of 107.0 kPa?
19. What volume of SO2 is produced from 32.5 g of ZnS at 23°C
and 103.3 kPa? ZnS + O2  ZnO + SO2
20. What is the temperature of CO2 gas when it has a density
of 0.0552 g/L and a pressure of .973 kPa?
VOCAB: Kelvin
STP
VOCAB:
solvation
Dissociation
percent by mass
solubility
ionization
Extra practice problems
Chapter 12
1.
What relationships can be determined from a balanced chemical equation?
2.
Explain why mole ratios are central to stoichiometric calculation
3. Silver nitrate and sodium phosphate are reacted in equal amounts of 200.0 g each.
How many grams of silver phosphate are produced?
3AgNO3 + Na3PO4 → Ag3PO4 + 3NaNO3
4a. What volume of hydrogen at STP is produced from the reaction of 50.0 g of Mg and 75.0 g of HCl?
Mg + 2HCl → MgCl2 + H2
b. How much excess reactant is left over?
5. A balloon is filled with 3.0 L of helium at 1 atm. What is the volume when the balloon rises
to an altitude where the pressure is only 0.25 atm? (assume temperature remains constant.)
6. The gas left in a used aerosol can is at a pressure of 1 atm at 27°C. If this can is thrown into a
fire, what is the internal pressure of the gas when its temperature reaches 927°C?
7. 5.2 L of a gas is at STP. Find the new volume when the temperature rises to 38°C and the
pressure drops to 600 mmHg.
8. Pressure and volume of a gas at constant temperature are __________________ proportional.
Why? ________________________________________________________________________
9. Volume and temperature of a gas at constant pressure are __________________ proportional.
Why? _____________________________________________________________
10. Volume and number of gas particles at constant pressure and temperature are
___________________ proportional.
11. If two containers are at the same temperature and pressure and their volumes are equal, they
must contain the same ________________________________. Which scientist said this?
__________________________
12. Which travels faster CO2 or O2? How much faster?
13. Gas A travels 4 times faster than Gas B. If the molar mass of Gas B is 80 g/mole, find the
molar mass of Gas A.
14. Refer to the phase diagram below when answering the questions:
a. What is the normal freezing point of this substance? ________
b. What is the physical state of this substance at 300°C and 0.50 atm ? ____________
c. If I had a quantity of this substance at a pressure of 1.25 atm and a temperature of 3000 C
and lowered the pressure to 0.25 atm, what phase transition(s) would occur? __________
15. Given the following boiling point data, if the same amount of liquid of each substance was
poured into separate, closed flasks at constant temperature, which substance would have the
lowest vapor pressure?
Formula of
Boiling
Name of compound
compound
Point (°C)
Water
H2O
100
Methanol
CH3OH
65
Ethanol
CH3CH2OH
78.5
Diethyl ether
CH3CH2OCH2CH3
34.5
Ethylene glycol
HOCH2CH2OH
198
a.
b.
c.
d.
e.
Water
Methanol
Ethanol
Diethyl ether
Ethylene glycol
16. At 1.0 atm , 0.75g of gas dissolves in 1L at 55 degrees. How much of the gas will dissolve in
4.0 atm at the same temperature? Who came up with this law?___________________________
17.
What volume of 3.7 M solution can be prepared using 89.5 grams of sulfuric acid?
18. What mass of magnesium chloride is required to prepare 2.15 liters of 6.5 M solution?
19. How would you prepare 2250 mL of a 3.25 M solution from a 16.0 M HNO3 stock solution?
20. If you mixed the following solutions, what would be the resulting molarity?
525 mL of 2.1M HCl
375 mL of 4.8 M HCl
295 mL of 7.6 M HCl
21. Circle all solutes that an “i” factor of 1. Why?
a. C6H12O6
b. CF4
c. NH4Cl
d. NH3
22. Why is calcium chloride more effective as rock salt in the winter than sodium chloride?