1. Properties of Gases
In organized soccer, a ball that is properly inflated will rebound faster and travel farther than a ball that is under-inflated. If the pressure is too high, the ball may burst when it is kicked. You will study variables that affect the pressure of a gas.

2. Compressibility
Compressibility
Why are gases easier to compress than solids or liquids are?

3. Compressibility
Compressibility is a measure of how much the volume of matter decreases under pressure. When a person collides with an inflated airbag, the compression of the gas absorbs the energy of the impact.
A crash dummy can be used to test the effectiveness of an air bag. Because gases can be compressed, the air bag absorbs some of the energy from the impact of a collision. Air bags work best when combined with seat belts.

4. Under pressure, the particles in a gas are forced closer together.
Compressibility
Gases are easily compressed because of the space between the particles in a gas.
The distance between particles in a gas is much greater than the distance between particles in a liquid or solid.
Under pressure, the particles in a gas are forced closer together.

5. Compressibility
At room temperature, the distance between particles in an enclosed gas is about 10 times the diameter of a particle.
There are only a few nitrogen and oxygen molecules in this model of air. At room temperature, the distance between molecules in a container of air at standard pressure is about 10 times the diameter of a molecule.

6. Factors Affecting Gas Pressure
What are the three factors that affect gas pressure?

7. Factors Affecting Gas Pressure
The amount of gas, volume, and temperature are factors that affect gas pressure.

8. Factors Affecting Gas Pressure
Four variables are generally used to describe a gas. The variables and their common units are
pressure (P) in kilopascals
volume (V) in liters
temperature (T) in kelvins
the number of moles (n).

9. Factors Affecting Gas Pressure
Amount of Gas
You can use kinetic theory to predict and explain how gases will respond to a change of conditions. If you inflate an air raft, for example, the pressure inside the raft will increase.

10. Factors Affecting Gas Pressure
Collisions of particles with the inside walls of the raft result in the pressure that is exerted by the enclosed gas. Increasing the number of particles increases the number of collisions, which is why the gas pressure increases.
The volume of this air-filled raft is much larger than its volume before it was inflated. Using a pump to force air into a raft increases the pressure of the air inside the raft. The increased pressure causes the raft to inflate to its intended size.

11. Factors Affecting Gas Pressure
If the gas pressure increases until it exceeds the strength of an enclosed, rigid container, the container will burst.
When a gas is pumped into a closed rigid container, the pressure increases as more particles are added. If the number of particles is doubled, the pressure will double. Predicting What would happen to the pressure in the container if the number of particles were tripled? If the number of particles were cut in half?

12. Factors Affecting Gas Pressure
Aerosol Spray Paint
The pressure of the gas inside a new can of spray paint is greater than the air pressure outside the can. When gas rushes though an opening in the top of the can, it propels, or forces, paint out of the can. As the can is used, the pressure of the propellant decreases. Relating Cause and Effect What happens when the pressure of the propellant equals the air pressure outside the can?

13. Factors Affecting Gas Pressure
Volume
You can raise the pressure exerted by a contained gas by reducing its volume. The more a gas is compressed, the greater is the pressure that the gas exerts inside the container.

14. Factors Affecting Gas Pressure
When the volume of the container is halved, the pressure the gas exerts is doubled.
A piston can be used to force a gas in a cylinder into a smaller volume. When the volume is decreased, the pressure the gas exerts is increased. Interpreting Diagrams What happens to the gas pressure when the volume is reduced from 1 L to 0.5 L?

15. Factors Affecting Gas Pressure
Temperature
An increase in the temperature of an enclosed gas causes an increase in its pressure.
As a gas is heated, the average kinetic energy of the particles in the gas increases. Faster-moving particles strike the walls of their container with more energy.

16. Factors Affecting Gas Pressure
When the Kelvin temperature of the enclosed gas doubles, the pressure of the enclosed gas doubles.
An increase in temperature causes an increase in the pressure of an enclosed gas. The container can explode if there is too great an increase in the pressure.

17. Chemistry 14.2

18. The Gas Laws
This hot air balloon was designed to carry a passenger around the world. You will study some laws that will allow you to predict gas behavior under specific conditions, such as in a hot air balloon.

19. Boyle’s Law: Pressure and Volume
How are the pressure, volume, and temperature of a gas related?

20. Boyle’s Law: Pressure and Volume
If the temperature is constant, as the pressure of a gas increases, the volume decreases.

21. Boyle’s Law: Pressure and Volume
Boyle’s law states that for a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure.

22. Boyle’s Law: Pressure and Volume
The pressure of a gas changes as the volume changes. INTERPRETING GRAPHS a. Observing When the volume is 2.0 L, what is the pressure? b. Predicting What would the pressure be if the volume were increased to 3.0 L? c. Drawing Conclusions Based on the shape of the graph, describe the general pressure-volume relationship.

23. Boyle’s Law: Pressure and Volume
Simulation 15
Examine the relationship between gas, volume and pressure.

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29. Charles’s Law: Temperature and Volume
As the temperature of an enclosed gas increases, the volume increases, if the pressure is constant.

30. Charles’s Law: Temperature and Volume
As the temperature of the water increases, the volume of the balloon increases.
When the gas in the blue balloon is cooled at constant pressure, the volume of the gas decreases. When the gas is heated at constant pressure, the volume increases. Calculating What is the ratio of volume to temperature for each set of conditions? Round your answer to two significant figures.

31. Charles’s Law: Temperature and Volume
Charles’s law states that the volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant.

32. Charles’s Law: Temperature and Volume
This graph shows how the volume changes as the temperature of a gas changes. INTERPRETING GRAPHS a. Observing What is the unit of temperature? b. Drawing Conclusions What happens to the volume as the temperature rises? c. Predicting If the temperature of a gas were 0 K, what would the volume of the gas be?

33. Charles’s Law: Temperature and Volume
Simulation 16
Examine the relationship between gas volume and temperature.

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39. Gay-Lussac’s Law: Pressure and Temperature
As the temperature of an enclosed gas increases, the pressure increases, if the volume is constant.

40. Gay-Lussac’s Law: Pressure and Temperature
When a gas is heated at constant volume, the pressure increases.
When a gas is heated at constant volume, the pressure increases. Interpreting Diagrams How can you tell from the drawings that there is a fixed amount of gas in the cylinders?

41. Gay-Lussac’s Law: Pressure and Temperature
Gay-Lussac’s law states that the pressure of a gas is directly proportional to the Kelvin temperature if the volume remains constant.

42. Gay-Lussac’s Law: Pressure and Temperature
A pressure cooker demonstrates Gay- Lussac’s Law.
In a pressure cooker, food cooks faster than in an ordinary pot with a lid.

43. Gay-Lussac’s Law: Pressure and Temperature
Simulation 17
Examine the relationship between gas pressure and temperature.

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48. for Sample Problem 14.3

49. The Combined Gas Law
The Combined Gas Law
When is the combined gas law used to solve problems?

50. The Combined Gas Law
The combined gas law describes the relationship among the pressure, temperature, and volume of an enclosed gas.

51. The Combined Gas Law
The combined gas law allows you to do calculations for situations in which only the amount of gas is constant.

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57. The Combined Gas Law
Weather balloons carry data-gathering instruments high into Earth’s atmosphere. At an altitude of about 27,000 meters, the balloon bursts.
Weather balloons carry instruments that can gather data about Earth’s atmosphere. Predicting Explain why helium is more likely than air to be used in weather balloons.

58. Ideal Gases
Solid carbon dioxide, or dry ice, doesn’t melt. It sublimes. Dry ice can exist because gases don’t obey the assumptions of kinetic theory under all conditions. You will learn how real gases differ from the ideal gases on which the gas laws are based.

59. Ideal Gas Law
Ideal Gas Law
What is needed to calculate the amount of gas in a sample at given conditions of volume, temperature, and pressure?

60. Ideal Gas Law
To calculate the number of moles of a contained gas requires an expression that contains the variable n.

61. The ideal gas constant (R) has the value 8.31 (L·kPa)/(K·mol).
Ideal Gas Law
The gas law that includes all four variables—P, V, T, and n—is called the ideal gas law.
The ideal gas constant (R) has the value (L·kPa)/(K·mol).

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67. Ideal Gases and Real Gases
Under what conditions are real gases most likely to differ from ideal gases?

68. Ideal Gases and Real Gases
There are attractions between the particles in an ideal gas. Because of these attractions, a gas can condense,or even solidify, when it is compressed or cooled.
In this flask used to store liquid nitrogen, there are two walls with a vacuum in between.

69. Ideal Gases and Real Gases
Real gases differ most from an ideal gas at low temperatures and high pressures.

70. Ideal Gases and Real Gases
This graph shows how real gases deviate from the ideal gas law at high pressures. INTERPRETING GRAPHS a. Observing What are the values of (PV)/(nRT) for an ideal gas at 20,000 and 60,000 kPa? b. Comparing What variable is responsible for the differences between the two (CH4) curves? c. Making Generalizations How does an increase in pressure affect the (PV)/(nRT ) ratio for real gases?

71. Gases: Mixtures and Movements
A list of gear for an expedition to Mount Everest includes climbing equipment, ski goggles, a down parka with a hood, and most importantly compressed-gas cylinders of oxygen. You will find out why a supply of oxygen is essential at higher altitudes.

72. Dalton’s Law
Dalton’s Law
How is the total pressure of a mixture of gases related to the partial pressures of the component gases?

73. Dalton’s Law
The contribution each gas in a mixture makes to the total pressure is called the partial pressure exerted by that gas.

74. Dalton’s Law
In a mixture of gases, the total pressure is the sum of the partial pressures of the gases.

75. Dalton’s Law
Dalton’s law of partial pressures states that, at constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases.

76. Observe the behavior of a mixture of nonreacting gases.
Dalton’s Law
Animation 17
Observe the behavior of a mixture of nonreacting gases.

77. Three gases are combined in container T.
Dalton’s Law
Three gases are combined in container T.
Three gases are combined in container T. The pressure that each gas exerts is independent of the pressure exerted by the other two gases. The pressure in container T is the sum of the pressures in containers A, B, and C. Interpreting Diagrams What is the relationship between the number of particles in containers A and C and the partial pressures of the gases in A and C?

78. Dalton’s Law
The partial pressure of oxygen must be kPa or higher to support respiration in humans. The climber below needs an oxygen mask and a cylinder of compressed oxygen to survive.
This climber is using a tank of compressed gas to supplement the supply of oxygen available at high altitudes.

79. 14.6
Firefighters carry tanks of compressed air. The tanks contain from 19.5% to 23.5% oxygen by volume.

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84. Graham’s Law
Graham’s Law
How does the molar mass of a gas affect the rate at which the gas effuses or diffuses?

85. Graham’s Law
Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout.

86. Graham’s Law
Bromine vapor is diffusing upward through the air in a graduated cylinder.
The diffusion of one substance through another is a relatively slow process. a) Bromine vapor is diffusing upward through the air in a graduated cylinder. b) After several hours, bromine vapors are near the top of the cylinder. Predicting What will happen as the bromine continues to diffuse?

87. Graham’s Law
After several hours, the bromine has diffused almost to the top of the cylinder.
The diffusion of one substance through another is a relatively slow process. a) Bromine vapor is diffusing upward through the air in a graduated cylinder. b) After several hours, bromine vapors are near the top of the cylinder. Predicting What will happen as the bromine continues to diffuse?

88. During effusion, a gas escapes through a tiny hole in its container.
Graham’s Law
During effusion, a gas escapes through a tiny hole in its container.
Gases of lower molar mass diffuse and effuse faster than gases of higher molar mass.

89. Thomas Graham’s Contribution
Graham’s Law
Thomas Graham’s Contribution
Graham’s law of effusion states that the rate of effusion of a gas is inversely proportional to the square root of the gas’s molar mass. This law can also be applied to the diffusion of gases.

90. Comparing Effusion Rates
Graham’s Law
Comparing Effusion Rates
A helium filled balloon will deflate sooner than an air-filled balloon.
The character balloons used in parades are filled with helium gas so that they will float.

91. Graham’s Law
Helium atoms are less massive than oxygen or nitrogen molecules. So the molecules in air move more slowly than helium atoms with the same kinetic energy.

92. Graham’s Law
Because the rate of effusion is related only to a particle’s speed, Graham’s law can be written as follows for two gases, A and B.

93. Graham’s Law
Helium effuses (and diffuses) nearly three times faster than nitrogen at the same temperature.