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Unit 8: Gases

TermDefinition
Pressure The amount of force exerted per unit area of a surface.
Newton The SI unit for force; the force that will increase the speed of a 1 kg mass by 1 m/s each second that the force is applied (abbreviation, N).
Barometer An instrument that measures atmospheric pressure.
Millimeters of Mercury A unit of pressure.
Atmosphere of Pressure The pressure of Earth's atmosphere at sea level; exactly equivalent to 760 mm Hg.
Pascal The SI unit of pressure; equal to the force of 1 N exerted over an area of 1 m2 (abbreviation, Pa)
Partial Pressure The pressure of each gas in a mixture.
Dalton's law of Partial Pressure The law that states that the total pressure of a mixture of gases is equal to the sum of the partial pressure of the component gases.
Boyles Law The law that states that for a fixed amount of gas at a constant temperature, the volume of the gas.
Absolute Zero The temperature at which all molecular motion stops (0 K on the Kelvin scale or -273.16 C on the Celsius scale).
Charle's Law The law that states that for a fixed amount of gas at a constant pressure, the volume of the gas increases as the temperature of the gas increases and the volume of the gas decreases as the temperature of the gas decreases.
Gay-Lussac's Law The law that states that the volume occupied by a gas at a constant pressure is directly proportional to the absolute temperature.
Combined Gas Law The relationship between the pressure, volume, and temperature of a fixed amount of gas.
Avogadro's Law The law that states that equal volume of gases at the same temperature and pressure contain equal numbers of molecules.
Standard Molar Volume of a Gas The volume occupied by one mole of a gas at STP is known as the standard molar mole of gas.
Ideal Gas Law The law that states the mathematical relationship of pressure (P), volume (V), temperature (T), the gas constant (R), and the number of moles of a gas (n); PV = nRT.
Ideal Gas Constant The proportionality constant that appears in the equation of state for 1 mole of an ideal gas; R = 0.082 057 84 L . K
Graham's Law of Effusion The law that states that the rate of effusion of a gas is inversely proportional to the square root of the gas's density.
Created by: pg428739
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