How are real gases different from ideal gases?

Real gases differ from ideal gases because in a real gas,

A. The particles aren't always moving

B. The particles don't bounce off walls

C. The particles take up volume

A. Inter-molecular forces exist between particles

B. The average energy depends only on the temperature

C. The particles don't lose energy from collisions

Real gases differ from ideal gases because, in a real gas,

C. The particles take up volume

A. Inter-molecular forces exist between particles

Explanation:

The particles of an ideal gas have no volume and no attractions for each other.

In a real gas, however, the molecules do have a measurable (but small) volume. For example, the volume of 1 mol an ideal gas at STP (0 °C and 1 bar) is 22.711 L. The molar volume of a real gas would be slightly greater than 22.711 L.

The molecules of real cases have intermolecular attractions for each other. On average, they will be slightly closer to each other, so the molar volume of a real gas will be slightly less than 22.711 L.

However, real gases are like ideal gases because their molecules

are always moving have an average kinetic energy that depends only on the temperature have elastic collisions (no loss of energy) with each other and with the walls of the container

Real gases have small attractive and repulsive forces between particles and ideal gases do not real gas particles have a volume in ideal gas particles do not real gas particles Collide inelastically loses energy of collisions and ideal gas particles collide elastically