What Are The Main Postulates Of Kinetic Molecular Theory Of Gases?

Kinetic molecular theory explains the behavior of gases in terms of interaction of molecules and the energy they posses
The main postulates of K.M.T are as follows
1 any gas consists of large number of tiny particles called molecules. Molecules consist of an atom or group of atoms. All the molecules of a gas are in stability are considered to identical
2 a finite volume of gas consists of large number of molecules
3 the molecules are point masses. The distance between molecules is very large as compared to there own dimensions.

4 the molecules are in a state of continuos motion they move randomly in all directions
5 during their random motion at various speeds the molecules collide with each other and with the walls of the container. The collision is completely elastic
6 molecules exert negligible forces of attraction on each other except during collision
7 laws of mechanics by Newton are assumed to be true and applicable on the motion of molecules
8 the average transnational kinetic energy of molecules is directly proportional to the absolute temperature
9 molecules of gas exert pressure due to collision with the walls of vessel in which the are kept

Gases consists of small number of small particles called molecules. They are alike in shape and mass but are different from the molecules of other gases. They are in state of random motion. They are perfect elastic sphere.The force of attraction between molecules is negligible.There is no effect of gravity on them but they obeys newton's laws of motion. They are in a straight line of collision and the distance between the collision is called free path. The time period of molecules in negligible in comparison to the duration of collision.

The molecules of a gas have no forces of attraction for each other

This theory led Clausius to derive the kinetic equation and deduced all the gas laws from it. The theory was later on elaborated and extended by Maxwell, who gave the law of distribution of velocities.

According to Kinetic Molecular Theory, every gas consists of a large number of very small particles called molecules. The molecules of a gas move haphazardly, cool among themselves and with the walls of the container and change their directions. The pressure exerted by a gas is due to the collisions of its molecules with the walls of a container. The collisions among the molecules are perfectly elastic. The molecules of a gas are widely separated from one another and there are sufficient empty spaces among them. The molecules of a gas have no force of attraction for each other. The actual volume of molecules of a gas is negligible as compared to the volume of the gas.

The motion imparted to the molecules by gravity is negligible as compared to the effect of the continued collisions between them. The average kinetic energy of the gas molecules varies directly as the absolute temperature of the gas.

R.J. Clausius deduced an expression for the pressure of an ideal gas. Actually, pressure on the walls of the vessel is due to collisions. Whenever the molecules move they collide among themselves and with the walls of the container. Due to these collisions, a force is expressed on the walls of the container. This force when divided by the area of the vessel gives force per unit area, which is called pressure.