Question

The pressure of a real gas is less than the pressure of an ideal gas (keeping other conditions same). It is because of:

• A. increase in collisions in real gas
• B. increase in intermolecular forces in real gas
• C. finite size of molecules in real gas
• D. none of these

Answer 1

The correct option is B increase in intermolecular forces in real gas

Due to intermolecular forces between gas molecules, a gas molecule hitting the wall will not be able to hit it with full force. The molecules inside the volume will exert an attractive force on the molecule which is about to hit the wall of the container. As a result, the pressure of a real gas is less than that of a pressure of an ideal gas.

Hence, the correct option is $\text{B}$