Explain : Why real gases behave deviation than ideal gas ?

Explanation

We find that two assumptions of the kinetic theory do not hold good.
There is no force of attraction between the molecules of a gas : If assumption is correct, the gas will never liquify. However, we know that gases do liquify when cooled and compressed. Also, liquids formed are very difficult to compress. This means that forces of repulsdion are powerful enough ad prevent squashing of molecules in tiny volume.
`therefore` There must be attraction force present between molecules of gases.
Volume of the molecules of a gas is negligibly small in comparison to the space occupied by the gas : If assumption is correct, the presure vs volume graph of experimental data (real gas) and that theoretically calculated from Boyle.s law (ideal gas) should coincide But such thing is not possible so Assumptions are unfair.