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The Ideal Gas Law - Gases are highly compressible with changes in density directly related to changes in temperature and pressure. M i = the molar mass of each gas The Universal Gas Constant - R u - in alternative Units The average molecular weight of a gas mixture is equal to the sum of the mole fractions of each gas multiplied by the molecular weight of that particular gas: N A = Avogadro Number = 6.022 x 10 23 The Molecular weight of a Gas Mixture

K = Boltzmann's constant = 1.381 x 10 -23 The universal gas constant can be defined in terms of Boltzmann's constant k as: R u = M gas R The Universal Constant defined in Terms of the Boltzmann's Constant

The Universal Gas Constant - R u - appears in the ideal gas law and can be expressed as the product between the Individual Gas Constant - R - for the particular gas - and the Molecular Weight - M gas - for the gas, and is the same for all ideal or perfect gases: In the SI system the most common units are J/kg K. In the imperial system the most common units for the individual gas constant are ft lb/slug oR. The induvidual gas constant, R, for a gas can be calculated from the universal gas constant, R u ( given in several units below), and the gas molecular weight, M gas: The Individual Gas Constant depends on the particular gas and is related to the molecular weight of the gas. The Universal and Individual Gas Constants are known from the Ideal Gas Law.