Chapter 14 Review
“The Behavior of Gases”
Honors Chemistry
First Item: Know the
Theory and Definitions
of the Gas Laws
Remember
PTV
Chapter 14 Review
Charles’s law states that ____.
 As the temperature of a fixed volume of
a gas increases, the pressure will ____.
 Which gas law can be used to calculate
the number of moles of a contained
gas?
 If a sealed syringe is plunged into cold
water, in which direction will the syringe
piston slide?

Chapter 14 Review
An ideal gas CANNOT be ____.
 If the atmospheric pressure on Mt.
Everest is one-third the atmospheric
pressure at sea level, the partial
pressure of oxygen on Mt. Everest is __.
 Boyle’s law states that ____.
 Which of the following atoms would have
the greatest velocity if each atom had
the same kinetic energy?
a) ammonia, or b) hydrogen

Chapter 14 Review
 Why
does air escape from a tire
when the tire valve is opened?
 The tendency of molecules to move
from high concentration toward
areas of lower concentration is
called ____.
 What happens to the pressure of a
gas inside a container if the
temperature of the gas decreases?
Chapter 14 Review
 Which
of the following gases will
effuse the most rapidly?
a) chlorine, or b) hydrogen
 How does the gas propellant move
when an aerosol can is used?
 Under what conditions of
temperature and pressure is the
behavior of a real gas most like that
of an ideal gas?
Chapter 14 Review
 If
a sealed syringe is heated, in which
direction will the syringe plunger
move?
 The volume of a gas is doubled while
the temperature is held constant. So,
how does the gas pressure change?
 What does the ideal gas law allow a
scientist to calculate that the other gas
laws do not?
Chapter 14 Review
How is the ideal gas law usually written?
 The combined gas law relates which
items together?
 If a balloon is squeezed, what happens
to the pressure of the gas inside the
balloon?
 Which of the following gases is the best
choice for inflating a balloon that must
remain inflated for a long period of time:
a) argon, or b) hydrogen?

Chapter 14 Review
At low temperatures and pressures, how
does the volume of a real gas compare
with the volume of an ideal gas under
the same conditions?
 If the volume of a container of gas is
reduced, what will happen to the
pressure inside the container?
 In general, for a gas at a constant
volume, the pressure of the gas is ____
proportional to its Kelvin temperature.

Chapter 14 Review
 At
high pressures, how does the
volume of a real gas compare with
the volume of an ideal gas under the
same conditions?
 Why does the pressure inside a
container of gas increase if more
gas is added to the container?
 Why is a gas easier to compress
than a liquid or a solid?
Second Item: Know the
Math to solve the
Problem Calculations
Equations are on the board at the
front of the room.
Steps to Solve the Math
Calculations of the Gas Laws:
1) Carefully read the question; write down the
known and unknown values on your paper.
2) Choose the equation that contains the
known and unknown values.
3) Algebraically solve the equation for the
unknown value.
4) Insert the known values into the equation,
and carefully calculate the answer.
Chapter 14 Review
 The
gaseous product of a reaction
is collected in a 25.0 L container at
27 oC. The pressure in the
container is 300.0 kPa and the gas
has a mass of 96.0 g. How many
moles of the gas are in the
container?
Chapter 14 Review
A
balloon filled with helium has a
volume of 30.0 L at a pressure of 100
kPa and a temperature of 15.0 oC.
What will the volume of the balloon
be if the temperature is increased to
80.0 oC and the pressure remains
constant?
Chapter 14 Review
 The
volume of a gas is 250 mL at
340.0 kPa pressure. What will the
volume be when the pressure is
reduced to 50.0 kPa, assuming the
temperature remains constant?
 A gas occupies a volume of 140 mL
at 35.0 oC and 97 kPa. What is the
volume of the gas at STP?
Chapter 14 Review
A
gas has a volume of 590 mL at a
temperature of -55.0 oC. What
volume will the gas occupy if the
temperature changes to 30.0 oC?
 What is the pressure exerted by
32 g of O2 in a 22.0 L container at
30.0 oC?
Chapter 14 Review
A
rigid container of O2 has a
pressure of 340 kPa at a
temperature of 713 K. What is the
pressure at 273 K?
 A gas has a pressure of 710 kPa at
227 oC. What will its pressure be at
27 oC, if the volume does not
change?
Chapter 14 Review
Use Graham’s law to calculate how
much faster fluorine gas (F2) will
effuse than chlorine gas (Cl2). Use the
molar mass of F2 = 38.0; the molar
mass of Cl2 = 70.9.
 A gas storage tank has a volume of
3.5 x 105 m3 when the temperature is
27 oC and the pressure is 101 kPa.
What is the new volume of the tank if
the temperature drops to -10 oC and
the pressure drops to 95 kPa?

Chapter 14 Review
A 10 g mass of krypton occupies 15.0 L
at a pressure of 210 kPa. Find the
volume of the krypton when the pressure
is increased to 790 kPa.
 A mixture of gases at a total pressure of
95 kPa contains N2, CO2, and O2. The
partial pressure of the CO2 is 24 kPa and
the partial pressure of the N2 is 48 kPa.
What is the partial pressure of the O2?

Chapter 14 Review
 How
many moles of N2 are in a flask
with a volume of 250 mL at a
pressure of 300.0 kPa and a
temperature of 300.0 K?