10 . Kinetic Molecular theory :
o Gases consist of large number of identical particles ( atoms or molecules ) that are so small that the actual volume of the molecules is negligible in comparison to the empty space between them .
o There is no force of attraction between the particles of a gas at ordinary temperature and pressure
o Particles of a gas are always in constant and random motion
o Pressure is exerted by the gas as a result of collision of the particles with the walls of the container o Collisions of gas molecules are perfectly elastic
o At any particular time , different particles in the gas have different speeds and hence different kinetic energies
o Average kinetic energy of the gas molecules is directly proportional to the absolute temperature
11 . Real Gases : The gases which deviates from Ideal behavior at higher pressure and low temperature b / c of force of attraction b / w molecules increases .
12 . Compressibility factor ( Z ) : It determine extent of devation
of real gases from Ideal gas behavior : Z =
15 . Critical Pressure : The minimum pressure required to liquity a gas at its critical temperature .
PV n . R . T . for ideal gas Z = 1 , for Non ideal gas Z < 1 , Z > 1 n 2 a 13 . Vander waal ’ s Equation : P V nb nRT .
V 2 14 . Critical Temperature : ( Tc ) The temperature above which a gas cannot be liquefied whatever high pressure may be