compressibility gases are easily compressed because of the space between the particles in a gas. the...
TRANSCRIPT
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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.
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Factors Affecting Gas Pressure
The amount of gas, volume, and temperature are factors that affect gas pressure.
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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).
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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.
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Factors Affecting Gas Pressure
If the gas pressure increases until it exceeds the strength of an enclosed, rigid container, the container will burst.
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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.
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Factors Affecting Gas Pressure
When the volume of the container is halved, the pressure the gas exerts is doubled.
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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.
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Factors Affecting Gas Pressure
When the Kelvin temperature of the enclosed gas doubles, the pressure of the enclosed gas doubles.
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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.
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Boyle’s Law: Pressure and Volume
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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.
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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.
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The Combined Gas Law
The combined gas law describes the relationship among the pressure, temperature, and volume of an enclosed gas.
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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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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 8.31 (L·kPa)/(K·mol).
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14.5
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14.5
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for Sample Problem 14.5
Problem Solving 14.24
Solve Problem 24 with the help of an interactive guided tutorial.
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Ideal Gases and Real Gases
Ideal Gases and Real Gases
Under what conditions are real gases most likely to differ from ideal gases?
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Ideal Gases and Real Gases
a. 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.
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Ideal Gases and Real Gases
Real gases differ most from an ideal gas at low temperatures and high pressures.
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Ideal Gases and Real Gases
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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.
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Dalton’s Law
The contribution each gas in a mixture makes to the total pressure is called the partial pressure exerted by that gas.
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Dalton’s Law
a. Three gases are combined in container T.
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Graham’s Law
a. Bromine vapor is moving upward through the air in a graduated cylinder.
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Graham’s Law
a. After several hours, the bromine has moved almost to the top of the cylinder.
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Graham’s Law
Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout.
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Graham’s Law
a. 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.
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Graham’s Law
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.
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Graham’s Law
Comparing Effusion Rates
a. A helium filled balloon will deflate sooner than an air-filled balloon.
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Graham’s Law
a. 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.
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Graham’s Law
a. 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.
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Graham’s Law
a. Helium effuses (and diffuses) nearly three times faster than nitrogen at the same temperature.