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