The kinetic theory of gases is based on the following postulates:

1. Gases are made up of a large number of molecules:

   Gases consist of a very large number of identical molecules that are perfectly elastic point masses.

2. The molecules are in constant, random motion:

   Gas molecules are in constant, random motion, moving in straight lines until they collide with each other or with the walls of the container.

3. Collisions are perfectly elastic:

   Collisions between gas molecules and between the molecules and the walls of the container are perfectly elastic. This means that no kinetic energy is lost during collisions. Source

4. The volume of the molecules is negligible:

   The volume of the gas molecules is negligible compared to the total volume of the container.

5. There are no intermolecular forces:

   There are no attractive or repulsive forces between gas molecules.

6. The average kinetic energy depends on temperature:

   The average kinetic energy of the gas molecules is directly proportional to the absolute temperature of the gas. All gases have the same kinetic energy at a specified temperature.