Which of the following statements is true of the molecules of a gas under ideal conditions? The molecules

The statement that is true of the molecules of a gas under ideal conditions is that they move at random. In the kinetic theory of gases, it is assumed that gas molecules are in constant random motion, colliding with each other and the walls of their container. This movement is what gives gases their pressure, as the molecules collide with the walls of the container and exert a force. The other options are not true of ideal gases. Gas molecules under ideal conditions undergo perfectly elastic collisions, meaning they do not lose any kinetic energy during their collisions. They do not attract each other, as they are assumed to be point masses with no intermolecular forces, and they occupy a small volume, as they are assumed to have no volume themselves, but only occupy the space in the container they are in.