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| a measure of force exerted per unit area; in chemistry, most commonly the force exerted by gas molecules as they strike the surfaces around them |
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| millimeter of mercury (mmHG) |
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| a common unit of pressure referring to the air pressure required to push a column of mercury to a height of 1 mm in a barometer; 760 mmHG = 1 atm |
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| an instrument used to measure atmospheric pressure |
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| a unit of pressure based on the average pressure of air at sea level; 1 atm = 101,325 Pa |
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| an instrument used to determine the pressure of a gaseous sample, consisting of a liquid-filled U-shaped tube with one end exposed to the ambient pressure and the other end connected to the sample |
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| the law that states that volume of a gas is inversely proportional to its pressure |
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| the law that states that the volume of a gas is directly proportional to its temperature |
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| the law that states that the volume of a gas is directly proportional to its amount in mole |
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| the law that combines the relationship of Boyle's, Charles's, and Avogadro's laws into one comprehensive equation of state with the proportionally constant R in the form PV=nRT |
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| the proportionality constant of the ideal gas law |
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| standard temperature and pressure (STP) |
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| the conditions of T=0 degrees C (273 K) and P= 1 atm |
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| the volume occupied by one mole of gas; the molar volume of an ideal gas at STP is 22.4 L |
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| the pressure due to any individual component in a gas mixture |
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| Dalton's law of partial pressures |
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| the law stating that the sum of the partial pressures of the the components in a gas mixture must equal the total pressure |
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| a means of expressing solution concentration as the number of moles of solute per moles of solution |
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| a physiological condition caused by low levels of oxygen, marked by dizziness, headache, and shortness of breath and eventually unconsciousness of even death in severe cases |
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| a physiological condition caused by an increased level of oxygen in the blood, resulting in muscle twitching, tunnel vision, and convulsions |
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| a physiological condition caused by an increased partial pressure of nitrogen, resulting in symptoms similar to those of intoxication |
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| the partial pressure of a vapor in dynamic equilibrium with its liquid |
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| a model of an ideal gas as a collection of point particles in constant motion undergoing completely elastic collisions |
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| the average distance that a molecule in a gas travels between collisions |
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| the process by which a gas spreads through a space occupied by another gas |
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| the process by which a gas escapes from a container into a vacuum through a small hole |
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| the extrapolation of the ideal gas law that considers the effects of intermolecular forces and particle volume in a nonideal gas |
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