Term
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Definition
| a simplified model gas where the particles do not interact |
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Term
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Definition
| pressure (P) is inversely proportional to volume (V) |
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Term
| Charles' law (and Gay-Lussac's law) |
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Definition
| the volume (V) of a gas is directly proportional to its absolute temperature (T) |
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Term
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Definition
| states that at the same temperature and pressure, equal volumes of different gases contain an equal number of particles |
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Term
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Definition
the "equation of state" for an ideal gas, which combines all of the empirical gas laws above
-relates the thermodynamic proper ties of an ideal gas to each other |
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Term
| equation for ideal gas law |
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Definition
| "P V = n R T", where P is pressure, V is volume, n is moles, T is absolute temperature, and R is the gas law constant (0.082 L-atm/mol•K = 8.314 J/mol•K) |
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Term
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Definition
proportionality constant for the ideal gas law
0.082 L-atm/mol•K = 8.314 J/mol•K |
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Term
| Dalton' law (of partial pressures) |
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Definition
| each gas in a mixture exerts a "partial pressure" which adds to the others to give the total pressure |
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Term
| equation for Dalton' law (of partial pressures) |
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Definition
| "Ptotal = Σ Pi" where Pi = Xi Ptotal is the partial pressure of gas "i" |
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Term
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Definition
| stoichometry where one of the reactants and/or products is a gas |
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Term
| gas phase stoichiometry uses this instead of mass or moles |
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Definition
| uses partial pressures instead of usual mass or mole units to describe the amount of gaseous species |
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