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| defined as the ratio of force to surface area |
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| the force exerted by the gases surrounding the earth on earth's surface and on all surfaces of al objects |
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| an instrument that measures atmospheric pressure |
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| the pressure capable of supporting a column of mercury 760nm high in a barometer |
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| measurement of pressure also called torr |
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| an instrument for measuring the pressure exerted by a gas |
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| states that the volume of a given amount of a gases at constant temperature is inversely proportional to its pressure |
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| states that the volume of a fixed quantity of gase at constant pressure is directly proportional to its absolute temperature |
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| states that the volume of a gas at a given temperature and pressure is proportional to the quantity of the gas |
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| states that, as the absolute temperature of a fixed amount of gas increases, the pressure increases as long as the volume and quantity of the gas remain constant |
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| a gas whose behavior is predicted by the linear relations definied by Boyle's, Charles', Avagadro's, and Amonton's laws |
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| relates the pressure, volume, number or moles, and temperature of an ideal gas |
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| the numerical constant "R" in the ideal gas equation, it's value and units depend on the units used for the variables in the ideal gas equation |
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| based on the ideal gas law; used when one or more of the four gas variables are held constant while the remaining variables change |
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| Standard Temperature and Pressure |
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| a temperature of zero degrees celsius and a pressure of one atmosphere |
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| the volume occupied by one mole of a gas at STP; equal to 22.4 L |
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| the contribution to the total pressure made by a component gas in a gas mixture |
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| Dalton's Law of Partial Pressures |
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| states that the total pressure of any mixture of gases equals the sum of the partial pressures of each gas in the mixture |
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| the ratio of the number of moles of a component in a mixture to the total number of moles in a mixture |
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| a model that describes the behavior of gases; based on a set of assumptions, and all the equations that define the relations between pressures, volume, temperature, and number of moles of gases can be derived by the theory |
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| the square root of the average of the squared speeds of all the molecules; a molecule possessing the average kinetic energy moves at this speed |
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| the process by which a gas escapes from its container through a tiny hole into a region of lower pressure |
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| states that the rate of effusion of a gas is inversely proportional to the square root of its molecular mass |
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| the speed of one substance (usually a gas or liquid) through another |
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| attempts to account for the behavior of real gases by including experimental determined factors that quantify the contributions of molecular volume and intermolecular interactions to the properties of gases |
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