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24 Cards in this Set
- Front
- Back
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A measure of the frequency and energy of molecules colliding against the walls of a container |
Gas pressure |
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A volume of space that does not contain gas molecules |
Vacuum |
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The pressure exerted by molecules in the air |
Atmospheric pressure |
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An instrument for measuring atmospheric pressure |
Barometer |
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A unit of pressure equal to 1 mm Hg |
Torr |
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The statement that equal volumes of gases, under the same conditions of temperature and pressure, contain equal numbers of molecules |
Avogadro's Theory |
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A relationship between two variables such that when one variable doubles, the other variable halfs |
Inversely proportional |
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A relationship between two variables such that when one variable doubles, the other variable doubles |
Directly proportional |
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The statement that the pressure and volume of a gas are inversely proportional at constant temperature |
Boyle's Law |
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The statement that the volume and the Kelvin temperature of gas are directly proportional at constant pressure |
Charle's Law |
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The statement that the pressure and the Kelvin temperature of a gas are directly proportional at constant volume |
Gay-Lussac's Law |
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The statement that the pressure exerted by a gas is inversely proportional to it's volume and directly proportional to it's Kelvin temperature |
Combined gas law |
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The conditions of gas at 273 K and 760 mm Hg |
Standard temperature and pressure |
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The pressure exerted by gaseous molecules above a liquid in a sealed container when the rates of evaporation and condensation are equal |
Vapor Pressure |
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The statement that the pressure exerted by a mixture of gases is equal to the sum of the individual pressures exerted by each gas |
Dalton's law of partial pressures |
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The pressure exerted by an individual gas in a mixture of two or more gases |
Partial pressure |
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A technique for determining the volume of gas from the volume of water it displaces |
Volume by displacement |
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A theoretical description of gas molecules demonstrating ideal behavior |
Kinetic theory |
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A theoretical gas that obeys the kinetic theory under all conditions |
Ideal gas |
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A gas that deviates from ideal behavior at low temperature and high pressure |
Real gas |
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An impact between gas molecules with no change in total energy |
Elastic collision |
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The theoretical temperature at which the kinetic energy of a gas is zero |
Absolute zero |
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The principle stated by the relationship PV= nRT |
Ideal gas law |
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The proportionality constant R on the equation PV=nRT |
Ideal gas constant |
