Postulates of Kinetic Theory of Gases
Postulates of Kinetic Theory of Gases
The kinetic theory of gases explained the behavior of the gases. On the basis of extensive study on the behaviour of gases, Bernouli, Boltzman, Maxwell, Clausious and ohers gave the following main postulates of kinetic theory of gases-1. Every gas consists of large number of tiny particles called point masses i.e. the actual volume of molecules is negligible when compared to the total volume of the gas.
2. The gas molecules are always in a state of rapid zig-zag motion in all directions. These molecules collide with each other and with the walls of the container.
3. A molecule moves in a straight line with uniform velocity between two collisions.
4. The molecular collisions are perfectly elastic so that there is no net loss of energy when the gas molecules collide with one another or against the walls of the container.
5. There are no attractive forces operating between molecules or between molecules and the walls of the container in which the gas has been contained. The molecule move independently from one another.
6. The pressure of the gas is force per unit area exerted by the moving molecules collide with the walls of the container.
7. Gaseous molecules does not have potential energy i.e. all the energy of the gaseous molecules is kinetic.
8. The average kinetic energy of gas molecules is directly proportional to absolute temperature. This means that the average kinetic energy of molecules is the same at a given temperature.
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