Chapter 12: The Gaseous State of Matter
Name: ____________________________________
12.2: The Kinetic Molecular Theory (KMT)
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A general theory called the Kinetic Molecular Theory, or KMT, explains the behavior and properties of gases.
The KMT is based on the motion of particles called gas molecules.
A gas that behaves exactly as outlined by the KMT is known as an ________________ ___________.
*Does an ideal gas exist in real life?
The principal assumptions of the KMT:
1. Gases consist of ________________ ___________________________.
2. The distance between particles is large compared with the size of the particles themselves. ,AKA…
3.
4.
5.
6.
Gas particles do not ______________ nor ________________ one another.
Gas particles are in _________________________________________________, colliding frequently with one another and
with the walls of the container. These collisions with the walls cause the ______________________ exerted by the gas.
No energy is lost by the collision of a gas particle with another gas particle or with the walls of the container. Therefore,
all collisions are said to be “______________________________________”.
The _____________________________________ for particles is the same for all gases at the same temperature, and its
value is directly proportional to the Kelvin temperature.
Characteristics of Gases:
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Due to their molecular motion, gases have the property of Diffusion. Define and illustrate Diffusion:
12.3: Measurement of Pressure of Gases
Define Pressure:
Define Atmospheric Pressure:
@ sea level, atmospheric pressure is: ________________
The pressure exerted by a gas depends on:
1.
2.
3.
What instrument is used to measure atmospheric pressure? ____________________________ How does it work?
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What are the different units used to measure pressure? Write the conversion factors for each.
1.) Convert the pressure 740. mm Hg to atm:
2.) Convert the pressure 1.12 atm to torr:
12.4: Dependence of Pressure on Number of Molecules and Temperature
How is the pressure of a gas produced?
At a specific temperature and volume, the # of collisions depends on the # of gas molecules in the container.
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If we double the # of molecules in a container, what happens to the frequency of collisions and the pressure?
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When the temperature of a gas increases, what happens to the kinetic energy of the molecules?
12.5: Boyle’s Law
Robert Boyle determined the relationship between the pressure (P) and volume (V) of a particular quantity of a gas in the late
1600’s. This relationship is called Boyle’s Law.
Describe Boyle’s Law:
What is the equation for Boyle’s Law?
Draw the graph illustrating Boyle’s Law:
Where can we see Boyle’s Law in action?
Boyle’s Law Problems:
1.) Atmospheric pressure on the peak of Mt. Everest can be extremely low, which is why climbers need to bring oxygen tanks
for the last part of the climb. If the climbers carry 10.0 L oxygen tanks with an internal gas pressure of 3040 mm Hg, what will be
the volume of the gas when it is released from the tanks at the top of the mountain where the pressure is 150 mm Hg?
2.) Divers get “the bends” if they come up too fast because gas in their blood can expand, forming bubbles in their blood stream.
If a diver has 0.050 L of gas in his blood under a pressure of 250 atm, then rises instantaneously to a depth where his blood has a
pressure of 50.0 atm, what will the volume of gas in his blood be? Do you think this will harm the diver?
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12.6: Charles’ Law
J. A. C. Charles studied the effect of temperature (T) on the volume (V) of a gas in 1787.
Describe Charles’ Law:
What is the equation for Charles’ Law?
*ALL temperatures in this equation must be in what unit?
Draw the graph illustrating Charles’ Law:
How do we convert to this?
Where can we see Charles’ Law in action?
Charles’ Law Problems:
1.) The temperature inside my refrigerator is about 4.0°C. If I place a balloon in my fridge that initially has a temperature of 22°C
and a volume of 0.50 liters, what will be the volume of the balloon when it is fully cooled by my refrigerator?
2.) On hot days, you may have noticed that potato chip bags seem to “inflate”, even though they have not been opened. If I have
a 250 mL bag at a temperature of 19°C, and I leave it in my car which has a temperature of 60.0°C, what will the new volume of
the bag be?
12.7: Lussac’s Law
Lussac studied the relationship involving the pressure (P) and temperature (T) of a gas at a constant volume.
Describe Lussac’s Law:
What is the equation for Lussac’s Law?
Draw the graph illustrating Lussac’s Law:
Where can we see Lussac’s Law in action?
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Lussac’s Law Problems:
1.) The pressure inside a container of helium gas is 650. mm Hg at 25°C. If the sealed container is cooled down to 0.0°C, what
will the pressure be?
2.) A gas cylinder contains 40.0 L of gas at 45.0°C and has a pressure of 750. mm Hg. What will the pressure be if the
temperature is changed to 100.0°C?
12.8: Combined Gas Laws
To compare volumes of gases, common reference points of temperature and pressure were selected and called
_________________________________________________, or _____________ for short.
What are the values for standard temperature and pressures?
What is the combined gas law equation?
Combined Gas Law Problems:
1.) Given 20.0 L of ammonia gas at 5.0°C and 730. torr, calculate the volume at 50.0°C and 800. torr.
2.) The volume of a gas-filled balloon is 50.0 L at 20.0°C and 742 torr. What volume will it occupy at standard temperature and
pressure (STP)?
 Describe what happens in the “Soda Can” Demo and why this happens:
12.9: Dalton’s Law of Partial Pressures
What is a “partial pressure”?
Define Dalton’s Law of Partial Pressures:
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Dalton’s Law of Partial Pressure Problems:
1.) A container contains He at a pressure of 0.50 atm, Ne at a pressure of 0.60 atm, and Ar at a pressure of 1.30 atm. What is the
total pressure in the container?
12.11: Mole – Mass – Volume Relationships of Gases
Since a mole contains __________________________ molecules, a mole of one gas will have the same volume as a mole of any
other gas at the same temperature and pressure.
 The volume occupied by a mole of any gas at STP is ______________. This quantity is known as the
_____________________________________.
If the mass and the volume of a gas at STP are known, we can calculate its molar mass.
1.) If 2.20 L of a gas measured at STP has a mass of 3.23 g, what is the molar mass of the gas?
Which of the following gases could this be?
A.) N2
B.) CO2
C.) O2
2.) What is the molar mass of a gas if 16.0 L of the gas has a mass of 19.0 g at 765 torr and 20.0 ºC?
12.12: Density of Gases
The density, d, of a gas is equal to: ______________ / ___________________ and has the unit: ________________.
The density of a gas at STP can be determined multiplying the molar mass of the gas by ___________________________.
1.) Calculate the density of Cl2 at STP.
2.) Calculate the density of SO2 at STP.
12.13: Ideal Gas Law
Provide the equation for the Ideal Gas Law:
* The units are very specific!
P:
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V:
n:
T:
The variable, R, is referred to as the ______________________________ and equals _________________________.
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Ideal Gas Law Problems:
1.) What pressure will be exerted by 0.400 mol of a gas in a 5.00 L container at 17°C?
2.) A 23.8 L cylinder contains oxygen gas at 20.0°C and 732 mm Hg. How many moles of oxygen are in the cylinder?
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How many grams of oxygen are in the cylinder?
12.14: Gas Stoichiometry
Mole – Volume and Mass – Volume Calculations
Gas Stoichiometry Problems:
1.) What volume of oxygen (at STP) can be formed from 0.500 mol of potassium chlorate? Write the balanced equation first.
2.) How many grams of aluminum must react with sulfuric acid to produce 1.25 L of hydrogen gas at STP? Write the balanced
equation first.
3.) What volume of oxygen will react with 150. L of hydrogen to form water vapor? Write the balanced equation first.
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What volume of water vapor will be formed?
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12.14: Real Gases
An ideal gas obeys all of the gas laws outlined in the Kinetic Molecular Theory (KMT). But remember…ideal gases do NOT exist
in nature!
Deviations from the gas laws occur at ___________________________________ and ________________________________________.
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Why?
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Why?
Under what conditions does a real gas behave the most like an ideal gas?
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___________________________________________:
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___________________________________________:
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