Explanation: Ideal gases are based on a few assumptions:
Elastic collisions between ideal gas molecules occur.
Ideal gas molecules have no potential energy, so they are unaffected by intermolecular forces.
When compared to the volume of the container, the volume of ideal gas molecules is negligible.
The molecules of an ideal gas are spherical in shape.
The molecules of an ideal gas are all the same.
As a result, real gases differ from ideal gases in the following ways:
Inelastic collisions occur between real gas molecules.
Real gas molecules have potential energy, which means they are influenced by intermolecular forces.
The volume of actual gas molecules is NOT insignificant.
The molecules of real gases are not spherical in shape.
The molecules of real gases are not all identical.