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Chemistry ch. 10

Gases

TermDefinition
1 atm 760 mm Hg
Boyle's law P1V1 = P2V2
Charles's law V1/T1 = V2/T2
Gay-Lussac's law P1/T1 = P2/T2
combined gas law P1V1/T1 = P2V2/T2
Avogadro's law n1/V1 = n2/V2
ideal gas law PV = nRT
R 0.082057 L*atm/mol*K
standard temperature and pressure, STP a pressure of 1 atm and temperature of 273 K
ideal gas law with mass and molar weight PV = (m/MW) RT
molar volume of an ideal gas 22.4 L at STP
density of a gas at STP molar mass/molar volume
equation for density d = (PMM)/RT
partial pressure the pressure exerted by a component of an ideal gaseous mixture
Dalton's Law of Partial Pressure the total pressure of a gas mixture is the sum of the partial pressures of the components of the mixture
vapor pressure the partial pressure of any liquid in air that is saturated with the vapors of that liquid - increases as temperature increases and is not linear
mole fraction number of moles of 1 component in a mixture divided by the total number of moles
partial pressure equation mole fraction * the total pressure
Created by: imr36093
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