Kinetic theory of gases #Assumption

kinetic theory of gases

Assumption

A gas consist a large number of molecules which are perfecte elastic spheres 

The molecules of gas in a state of random motion. They move in all directions with different speeds. 

The size of the gas molecule is very small as compared to the distance between them. Hence, volume occupied by the molecules is negligible in comparison to in volume of the gas. 

The molecules do not exert any force of attraction or repulsion on each other except during collision 

The collision of the molecules with themselves with walls of the container are perfectly elastic. 

There is no concentration of the molecule at any point inside the container i.e. molecular density is uniform through out the gas. 

A molecule move along a straight line between two successive collision and average Straight distance covered between two successive collision is called "mean free path" of the molecule.

The collision are almost instantaneous.