Kinetic Theory of Gases - II

Assumptions of Kinetic Theory of Gases

1. All gases consist of molecules which are rigid, elastic spheres identical in all respect for a given gas.

2. The size of a molecule is negligible as compared with the average distance between two molecules.

3. During the random motion, the molecules collide with one another and with the wall of the vessel.The collisions are almost instantaneous.

4. The molecular density remains uniform throughout the gas.

5. The collisions are perfectly elastic in nature and there are no forces of attraction or repulsion between them.

Pressure exerted by gas: 

Average Kinetic energy of a gas: If M is molecular mass and V is molecular volume
and m is mass of each molecule. Then
1. Mean K.E per mole of a gas,

Avogadro Law: Equal volume of all gases under similar condition of temp. and
pressure contain equal number of molecules

Avogadro Number: 

NA = 6.0225 x 10²³ mol^-1

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