From the experimental observations
p-v-T behaviour of the gases given by,
pṽ = ṜT
Where Ṝ is the universal
gas constant value of Ṝ is 8.3141 J / mol K
ṽ is the molar specific volume m3/gmol
Dividing upper equation
by the molecular weight µ.
pv
= RT
Where v is specific
weight m3/gmol
R is the characteristic
gas constant
We also get this the equation in terms of total volume V of gas,
PV = nṜT
PV = mRT
Where n is the number of
moles and m is the mass of the gas. An equation can be written for two states of
the gas is
P1V1 /
T1 = P2V2 / T2
All equation is called
the ideal gas equation of state. At very low pressure or density, all gases and
vapours approach ideal gas behaviour.