Gas laws, the ideal gas law, and partial pressures
Four variables describe a gas: pressure (P), volume (V), temperature (T, always in kelvins), and amount in moles (n). Holding the others constant, pressure and volume are inversely related (Boyle's law: P1V1 = P2V2), volume is directly proportional to Kelvin temperature (Charles's law), pressure is directly proportional to Kelvin temperature (Gay-Lussac's law), and volume is directly proportional to moles (Avogadro's law). The ideal gas law combines them: PV = nRT, where R is the gas constant, 0.0821 L atm per mol K. At standard temperature and pressure (0 degrees Celsius and 1 atmosphere), one mole of an ideal gas takes up about 22.4 liters. Dalton's law of partial pressures says that in a gas mixture, the total pressure is the sum of each gas's own partial pressure.
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