According to the kinetic molecular theory, gas particles are in constant motion and collide with each other and the walls of their container.

In the kinetic molecular theory, temperature is directly related to the average kinetic energy of the particles in a substance.

The kinetic molecular theory explains the behavior of solids, liquids, and gases.

According to the kinetic molecular theory, the distance between gas particles is relatively large compared to the size of the particles themselves.

According to the kinetic molecular theory, pressure is caused by particles colliding with the walls of their container.

In the kinetic molecular theory, liquids have particles that are much closer together than gases but still have some space to move.

The kinetic molecular theory states that as the temperature of a gas decreases, its particles move slower and have lower kinetic energy.

In the kinetic molecular theory, the particles of a gas are assumed to have no attractive forces between them.

Kinetic molecular theory explains that the average kinetic energy of gas particles is directly proportional to the temperature measured in Kelvin.

According to the kinetic molecular theory, particles in a solid vibrate around fixed positions but do not move freely.