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19 Cards in this Set
- Front
- Back
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Pressure |
The amount of force exerted per unit area of a substance. |
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Newton |
The SI for force; the force that will increase the speed of a 1kg mass by 1m/s each second that force is applied (abbreviation N) |
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Barometer |
An instrument that measures atmospheric pressure |
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Millimeters of mercury |
A unit of pressure |
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Atmosphere of pressure |
The pressure of earths atmosphere at sea level; exactly equivalent to 760 mmHG |
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Pascal |
The SI unit of pressure; equal to the force of 1 N exerted over an area of 1 m2 (abbreviation, Pa) |
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Partial Pressure |
The pressure of each gas in a mixture. |
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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 pressures of the component gases |
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Boyle's Law |
The law that states that for a fixed amount of gas at a constant temperature, the volume of the gas increases as the pressure of the gas decreases and the volume of the gas decreases as the pressure of the gas increases |
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Absolute Zero |
The temperature at which all molecular motion stops (0 k on the kelvin scale or -276.16 on Celsius scale) |
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Charles's Law |
The law that states that the volume occupied by a 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 decreases |
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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 |
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Combined gas law |
The relationship between the pressure, volume, and temperature of a fixed amount of gas |
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Gay-Lussac's law if combining volumes of gases |
The law that states that the volumes of gases involved in a chemical change can be represented by a ratio of small whole numbers |
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Avogadro's las |
The law that states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. |
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Standard molar volume of a gas |
The volume occupied by one mole of a gas at STP |
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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 |
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Ideal Gas Constant |
The proportionality constant that appears in the equation of state for 1mol of an ideal gas; R=0.082 057 841• atm/mol• k |
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Grahams 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 |
