At a high pressure, the compressibility factor (Z) of a real gas is usually greater than one. This can be explained from van der Waals equation by neglecting the value of:

At high pressure, the compressibility factor for one mole of van der waals gas will be

At high pressure, the compressibility factor for one mole of van der Waals gas will be

A: At very high pressures, compressibility factor is greater than 1. R: At very high pressure, 'b' can be neglected in van der Waals gas equation

Compressibility factor (Z) for a van der Waals real gas at critical point is

The van der Waals' equation for equal real gas is :

At high pressure, van der Waal's equation becomes:

The van der Waals' equation for a real gas is:

The behaviour of a real gas is usually depicted by plotting compressibility factor Z versus P at a constant temperature At high temperature and high pressure Z is usually more than one This fact can be explained by van der Waals' equation when .

The behaviour of a real gas is usually depicted by plotting compressibility factor Z versus P at a constant temperature. At high temperature and high pressure, Z is usually more than one. This fact can be explained by van der Waals equation when