The important postulates of Kinetic theory of gases are:
(i) All gases are made up of a very large number of minute particles called molecules.
(ii) The molecules are separated from one another by large distances. The empty spaces among the molecules are so large that the actual volume of the molecules is negligible as compared to the total volume of the gas.
(iii) The molecules are in a state of constant rapid motion in all the directions. During their motion, they keep on colliding with one another and also with the walls of the container and thus, change their directions.
(iv) Molecular collisions are perfectly elastic, i.e., no loss of energy occurs when the molecules collide with one another or with the walls of the container. However, there may be redistribution of energy during the collisions.
(v) There are no forces of interaction (attractive or repulsive) between molecules. They move completely independent of one another.
(vi) The pressure exerted by the gas is due to the bombardment of its molecules on the walls of the container per unit area.
(vii) The average kinetic energy of the gas molecules is directly proportional to the absolute temperature.
