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Kinetic Theory of Gases:

The various assumptions of the kinetic theory of gases are as follows:

a. A gas consists of a large number of tiny particles called molecules. The molecules of a gas are identical but differ from those of other gases. These molecules are perfectly rigid and perfectly elastic.

b. The size of a molecule is negligible compared with the average distance between the molecules.

c. The molecules are in a state of continuous random motion, moving in all directions with all possible velocities.

d. The molecules have velocities ranging from zero to infinity, so that the average velocity of random motion is zero.

e. The collision between two molecules is perfectly elastic, that is, the kinetic energy remains conserved in collision.

f. There is no inter molecular force of interaction between the molecules of the gas.

g. Between two successive collisions a molecule traverses a straight-line path with constant speed called the free path of the molecule.

h. The collisions are almost instantaneous that is, the duration of a collision is negligible as compared to time spent by a molecule between collisions.