1. Gases are composed of tiny particles (atoms or molecules) Gases are relatively small with relatively low atomic and molecular weights.

2. The gas particles are so small when compared to the distances between them, that their volume is negligible (assumed to be zero). There is a lot of space between the gas particles which explains gases compressibility (ability to be squeezed together)

3.The gas particles are in constant random motion, moving in straight lines and colliding with the inside walls of the container.

Gas particles move in straight lines and in all directions uniformly until they collide with something: another particle or the wall of the container they are in. This is why gases exert pressure on the walls of the container they are held in.

4. Gas particles are assumed to have negligible attractive or repulsive forces between each other. Their attraction and repulsion forces can be ignored (very little or weak – if any – IMF)

5. Gas particles may collide with each other in an elastic way, causing the total kinetic energy of the colliding particles not to change (Remain the same). Gas particles collide elastically thus the kinetic energy is not lost, but it may be transferred from one particle to the other.

6. The temperature (K°) is directly proportional to the average kinetic energy of the gas particles.

If a gas is heated so that the temperature increases, the average kinetic energy of the gas also increases, in other words the energy of motion of the gas particles increases proportionally.

	Created by Alejandra Gomez over 4 years ago

Chemistry 10th Slide Set on Kinetic molecular theory of gases KMT, created by Alejandra Gomez on 15/04/2020.