CoreChem:Kinetic Theory of Gases: The Total Molecular Kinetic Energy
Equation (1) from Postulates of the Kinetic Theory can tell us a lot more than this about gases, however. If both sides are multiplied by V, we have
The kinetic energy of an individual molecule is ½ m (u2)ave, and so the average kinetic energy (Ek)ave of a collection of molecules, all of the same mass m is
(Ek)ave = (½ m u2)ave = ½ m (u2)ave
The total kinetic energy Ek is just the number of molecules times this average:
Ek = N × (Ek)ave = N × ½ m (u2)ave
or, multiplying both sides by 3/3 (i.e., by 1)
Substituting from Eq.
The product of the pressure and the volume of a gas is two-thirds the total kinetic energy of the molecules of the gas. Now we can understand why PV comes out in joules—it is indeed energy. According to postulate 4 of the kinetic theory, gas molecules have constant total kinetic energy. This is reflected on the macroscopic scale by the constancy of PV, or, in other words, by Boyle's law. The kinetic theory also gives an important insight into what the temperature of gas means on a microscopic level. We know from the [[CoreChem:The Ideal Gas Equation|ideal gas law]] that PV = nRT. Substituting this into Eq. (3),
nRT = ⅔ Ek (4)
If we divide both sides of Eq. (4) by n and multiply by ,
The term Ek/n is the total kinetic energy divided by the amount of substance, that is, the molar kinetic energy. Representing molar kinetic energy Em by we have
The molar kinetic energy of a gas is proportional to its temperature, and the proportionality constant is times the gas constant R.