Real gases differ from ideal gases in that real gas particles have volume and collisions are not perfectly elastic, following gas laws only under certain conditions. Real gases can also liquefy under high pressure and have intermolecular attractive forces, while ideal gases are considered to have no volume, perfectly elastic collisions and no intermolecular forces between particles. Ideal gases follow gas laws under all temperature and pressure conditions.

1. Real vs. Ideal Gases

2. Real Gases If enough pressure is applied, the gas will turn into a liquid. All particles have the same volume. It follows laws under high pressures and low temperatures. The collisions are not elastic. They have polar intermolecular attractive forces.

3. Ideal Gases They take up no space. There are no intermolecular attractive forces. Particles are moving in constant, random motion. The collisions are elastic. There is no attraction or repulsion with the container. It follows laws under all conditions of temperature and pressure.