Question

Explain deviation of gases from ideal behaviour.

Answer 1

$\text{Deviation from ideal behavior}:$

$i)$ In case of ideal gas, it is assumed that, there no intersections between gas molecules.

$ii)$ The intermolecular distance between gas molecules is large as compared to size of the gas of molecule.

It is also believed that the actual volume occupied by the gas molecules is negligibly small as compared with the total volume of the gas.

$iii)$ These two assumptions are not strictly true. There are attractive forces of attraction called van der waal's forces. These interactive forces are responsible for liquefaction of gases.

$iv)$ Further, at relatively higher pressure, when total volume of gas becomes relatively small due to compression, the actual volume occupied by the gas molecules, though small can not be neglected.