Term
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Definition
| temperature at which the volume of a gas would be zero according to Charles?s law. |
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Term
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Definition
| (also, Gay-Lussac?s law) pressure of a given number of moles of gas is directly proportional to its kelvin temperature when the volume is held constant |
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Term
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Definition
| unit of pressure; 1 atm = 101,325 Pa |
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Term
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Definition
| volume of a gas at constant temperature and pressure is proportional to the number of gas molecules |
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Term
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Definition
| (bar or b) unit of pressure; 1 bar = 100,000 Pa |
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Term
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Definition
| device used to measure atmospheric pressure |
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Term
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Definition
| volume of a given number of moles of gas held at constant temperature is inversely proportional to the pressure under which it is measured |
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Term
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Definition
| volume of a given number of moles of gas is directly proportional to its kelvin temperature when the pressure is held constant |
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Term
| compressibility factor (Z) |
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Definition
| ratio of the experimentally measured molar volume for a gas to its molar volume as computed from the ideal gas equation |
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Term
| Dalton?s law of partial pressures |
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Definition
| total pressure of a mixture of ideal gases is equal to the sum of the partial pressures of the component gases. |
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Term
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Definition
| movement of an atom or molecule from a region of relatively high concentration to one of relatively low concentration (discussed in this chapter with regard to gaseous species, but applicable to species in any phase) |
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Term
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Definition
| transfer of gaseous atoms or molecules from a container to a vacuum through very small openings |
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Term
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Definition
| rates of diffusion and effusion of gases are inversely proportional to the square roots of their molecular masses |
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Term
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Definition
| pressure exerted by a fluid due to gravity |
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Term
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Definition
| hypothetical gas whose physical properties are perfectly described by the gas laws |
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Term
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Definition
| constant derived from the ideal gas equation?R?= 0.08206 L atm mol?1?K?1?or 8.314 L kPa mol?1?K?1 |
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Term
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Definition
| relation between the pressure, volume, amount, and temperature of a gas under conditions derived by combination of the simple gas laws |
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Term
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Definition
| theory based on simple principles and assumptions that effectively explains ideal gas behavior |
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Term
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Definition
| device used to measure the pressure of a gas trapped in a container |
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Term
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Definition
| average distance a molecule travels between collisions |
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Term
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Definition
| concentration unit defined as the ratio of the molar amount of a mixture component to the total number of moles of all mixture components |
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Term
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Definition
| pressure exerted by an individual gas in a mixture |
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Term
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Definition
| SI unit of pressure; 1 Pa = 1 N/m2 |
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Term
| pounds per square inch (psi) |
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Definition
| unit of pressure common in the US |
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Term
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Definition
| force exerted per unit area |
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Term
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Definition
| amount of gas diffusing through a given area over a given time |
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Term
| root mean square speed (urms) |
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Definition
| measure of average speed for a group of particles calculated as the square root of the average squared speed |
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Term
| standard conditions of temperature and pressure (STP) |
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Definition
| 273.15 K (0 degreeC) and 1 atm (101.325 kPa) |
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Term
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Definition
| volume of 1 mole of gas at STP, approximately 22.4 L for gases behaving ideally |
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Term
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Definition
| unit of pressure;?1 torr=1760atm1 torr=1760atm |
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Term
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Definition
| modified version of the ideal gas equation containing additional terms to account for non-ideal gas behavior |
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Term
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Definition
| pressure exerted by water vapor in equilibrium with liquid water in a closed container at a specific temperature |
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