QUARTER 3 EXAM REVIEW –March/April 2015
Chapter 9 – Stoichiometry
composition stoichiometry
limiting reactant
reaction stoichiometry
excess reactant
percent yield
theoretical yield
 Use the following equation to answer the questions that follow.
N2H4 (l) + H2O2 (l)  N2 (g) + H2O (g)
1. If 0.35 mol of N2H4 is used, how many moles of H2O2 is needed? How many moles of each
product are produced?
2. If 555 grams of water are produced, how many moles of H2O2 are needed?
3. If 1525 g of N2H4 are used, haw many grams of H2O2 are needed?
4. What is the limiting reactant if there are 500 g of N2H4 and 600 g of H2O2? How many grams of
teach product can be produced? If 550 g of water are actually produced, what is the percent yield?
Chapter 10 – States of Matter
fluid
capillary action
vaporization
freezing
supercooled liquids
equilibrium
Le Chatelier’s Principle
boiling point
molar heat of vaporization
triple point
critical pressure
kinetic molecular theory
effusion
surface tension
density
evaporation
melting
amorphous solid
phase
melting point
equilibrium vapor pressure
boiling
critical point
endothermic
ideal gas
diffusion
sublimation
compressibility
deposition
crystal
condensation
freezing point
volatile liquids
molar heat of fusion
critical temperature
exothermic
real gas
 Be able to identify the various phase changes and determine whether each process is
endothermic or exothermic.
1. How much heat must be added to 10.0 g of ice at –20.0oC to convert it to steam at 120.0oC?
2. Calculate the molar heat of fusion of a substance given that 0.433 mol of the substance absorbs
36.5 kJ of energy when it is vaporized.
3. How much energy is needed to vaporize 9.35 x 1024 molecules of water?
4. What is the molar mass of a 5510 g sample of a liquid that is allowed to freeze? As it freezes, the
substance releases 75.8 kJ of energy and the molar heat of fusion for this substance is 3.811 kJ/mol.
Chapter 11 –Gases
STP
force
Boyle’s Law
absolute zero
Dalton’s Law of Partial Pressure
Avogadro’s Principle
standard molar volume of a gas
pressure
ideal gas constant
Newton
barometer
Charles’ Law
Gay-Lussac’s Law
combined gas law
partial pressure
water displacement
Gay-Lussac’s Law of combining volumes
ideal gas law
 Know the various gas laws. What is the relationship between the variables in each law? What
is the constant in each law? What is the equation for each law?
 What temperature units MUST be used with all the gas laws?
1. If 500. mL of helium has a pressure of 2.4 atm, what will the pressure be if the gas is put into a
container that has a volume of 1200. mL? What law is represented by this situation?
2. A sample of neon gas has a volume of 852 mL at 25oC. What is the volume of the gas 50oC if the
pressure remains constant? What law is represented by this situation?
3. An aerosol can has a pressure of 3.00 atm at a temperature of 25oC. What will the pressure be if
the Celsius temperature doubles? What law is represented by this situation?
4. The volume of a gas is 35.0 mL at 20oC and 675 mmHg. What will the Celsius temperature be at
720 mmHg and a volume of 25.0 mL?
5. Convert 750. mmHg to:
A. Torr
B. Pascals
C. Atm
6. A 720.0 mL sample of hydrogen gas at 25.0oC and a pressure of 715 mmHg was collected by water
displacement. What volume will the dry gas occupy at STP?
7. What volume will be occupied by 0.525 mol of oxygen at STP?
8. What is the density of carbon monoxide at STP?
9. What is the molar mass of a gas that has a mass of 0.519 g and a volume of 200. mL at STP? Is the
gas propane (C3H8) or butane (C4H10)?
10. What is the volume in milliliters of 24.0 g of oxygen at 20.0 oC and 740 mmHg?
11. If 65.0 g of carbon are burned in the presence of oxygen to produce carbon monoxide at 27oC and
188 mmHg, how many liters of carbon monoxide are produced?
NOTE: THIS IS A REVIEW SHEET ONLY, AND ANYTHING COVERED THIS QUARTER
COULD BE ON THE QUARTER 3 ASSESSMENT. YOU SHOULD BE STUDYING THE
CHAPTERS IN THE TEXTBOOK, YOUR NOTES, AND WORKSHEETS WE HAVE DONE TO
HELP YOU PREPARE FOR THIS TEST.