Assumptions of Kinetic Theory of Gases
1 . Every gas consists of extremely small particles known as molecules . The molecules of a given gas are all identical but are different from those of another gas .
2 . The molecules of a gas are identical spherical , rigid and perfectly elastic point masses .
3 . Their molecular size is negligible in comparison to intermolecular distance ( 10 -9 m ).
4 . The speed of gas molecules lies between zero and infinity ( very high speed ).
5 . The distance covered by the molecules between two successive collisions is known as free path and mean of all free path is known as mean free path . 6 . The number of collision per unit volume in a gas remains constant . 7 . No attractive or repulsive force acts between gas molecules . 8 . Gravitational to extremely attraction among the molecules is ineffective due small masses and very high speed of molecules .
Gas laws
Assuming permanent gases to be ideal , through experiments , it was established that gases irrespective of their nature obey the following laws .
Boyle ’ s Law
At constant temperature the volume ( V ) of given mass of a gas is inversely proportional to its pressure ( p ), i . e ., V ∝ 1 / p ⇒ pV = constant
For a given geas , p1V1 = p2V2