INTRODUCTION TO KINETIC THEORY OF GASES
The kinetic theory of gases deals with the behaviour of molecules constituting the gas.
According to this theory, the molecules of all gases are in continuous motion. As a result of this they possess kinetic energy which is transferred from molecule to molecule during their collision. The energy so transferred produces a change in the velocity of individual molecules. The complete phenomenon of molecular behaviour is quite complex. The assumptions are therefore made to simplify the application of theory of an ideal gas.
KINETIC THEORY OF GASES ASSUMPTIONS
1. The molecules of gases are assumed to be rigid, perfectly elastic solid spheres, identical in all respects such as mass, form etc.
2. The mean distance between molecules is very large compared to their own dimensions.
3. The molecules are in state of random motion moving in all directions with all possible velocities and gas is said to be in state of molecular chaos.
4. The collisions between the molecules are perfectly elastic and there are no intermolecular forces of attraction or repulsion. This means that energy of gas is all kinetic.
5. The number of molecules in a small volume is very large.
6. The time spent in collision is negligible, compared to the time during which the molecules are moving independently.
7. Between collisions, the molecules move in a straight line with uniform velocity because of frictionless motion between molecules. The distance between two collisions is called ‘free path’ of the molecule, the average distance travelled by a molecule between successive collision is known as ‘mean free path’.
8. The volume of molecule is so small that it is negligible compared to total volume of the gas.Tags: Basic of kinetic theory of gases, Kinetic theory, Kinetic theory and thermodynamics, Kinetic theory of gases, Postulates of kinetic theory of gases