Identify false statement about real gas from following.

Real gases behave like ideal gases at high temperatures and low pressures, so they obey Boyle's and Charles' laws under these conditions.

Unlike the theoretical model of an ideal gas, where molecules are assumed to be rigid spheres that undergo perfectly elastic collisions , real gas molecules have internal structures and exert intermolecular forces on each other. When real gas molecules collide, some of their translational kinetic energy can be temporarily converted into internal energy, meaning the collisions themselves are not perfectly elastic.

Real gases have finite molecular volumes and exert intermolecular forces of attraction on each other.

Because of these intermolecular forces, when the temperature of a real gas is sufficiently lowered (reducing the kinetic energy of the molecules) and pressure is applied, the gas molecules come close enough together to condense into a liquid state.

The property of not being able to liquefy at any temperature applies strictly to an ideal gas, which is theoretically assumed to have zero intermolecular attraction.

Therefore, the statement that a real gas cannot liquefy even at low temperatures is false.

Answer: It can not liquify even at low temperature.