Chapter 14 Review *The Behavior of Gases*

Chapter 14 Review
“The Behavior of Gases”
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
Chapter 14 Review
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
 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
 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
 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?
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 .How many
moles of the gas are in the
container? (3 mol)
Chapter 14 Review
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? (36.8 L)
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
 A gas occupies a volume of 140 mL
at 35.0 oC and 97 kPa. What is the
volume of the gas at STP? (119 mL)
Chapter 14 Review
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?
 (820 mL)
 What is the pressure exerted by
32 g of O2 in a 22.0 L container at
30.0 oC? (1.13 atm)
Chapter 14 Review
rigid container of O2 has a
pressure of 340 kPa at a
temperature of 713 K. What is the
pressure at 273 K? (130 kPa)
 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? (440 kPa)
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. 1.37X
Chapter 14 Review
 How
many moles of N2 are in a flask
with a volume of 250 mL at a
pressure of 3 atm and a temperature
of 300.0 K? (0.03 mol)
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