From equation (5) we have
     PV = (1/3)Nmvmq2 
where N is the number of molecules in the sample. Above equation can also be written as
     PV = (2/3)N(1/2)Nmvmq2 (7)
The quantity (1/2)Nmvmq2 in equation (7) is the kinetic energy of molecules in the gas. Since the internal energy of an ideal gas is purely kinetic we have,
     E=(1/2)Nmvmq2 (8)
Combining equation 7 and 8 we get
Comparing this result with the ideal gas equation (equation (4) ) we get 
or,     E/N=(1/2)mvmq2 =(3/2)KBT 
Where, KB is known as Boltzmann constant and its value is KB=1.38 X 10-23 J/K
From equation (11) we conclude that the average kinetic energy of a gas molecule is directly proportional to the absolute temperature of the gas and is independent of the pressure , volume and nature of the gas.
Hence average KE per molecule is 
from this since v2¯=(vrms)2, rms velocity of a molecule is
     vrms=√(3KBT/m) (10)
This can also be written as
where, M=mN is the molecular mass of the gas.