Ideal gas equation strictly obeys gas laws under all conditions of

Real gases do not follow the ideal gas equation perfectly under all conditions . They show deviation from the ideal behavior when

A gas which obeys all the assumptions of kinetic theory of gases at all conditions of temperatures and pressures is called

The gases which strictly follow the general equation (PV = nRT) are called ideal or perfect gases. Actually, there is no gas which is perfect or ideal. A real gas is one which actually exists, whether it obeys gas laws strictly or not. Under ordinary conditions, only those gases nearly behave as ideal or perfect which have very low boiling points such as nitrogen, hydrogen ect. The most easily liquefiable and highly soluble gases such as ammonia, carbon dioxide, sulphur dioxide show large deviation A very convenient method of studying deviation of real gases from ideal behaviour is through a compressibility factor (Z) Z = (PV)/(nRT) (i) Z = 1 , for ideal gases. (ii) Z != 1 , for real gases. At Boyle's temperature, compressibility factor Z for a real gas is :

Ideal gas equation | Kinetic Theory of Gases | Pressure by gas on container | Translational Kinetic Energ | Degrees of freedom | Law of equipartition of energy | Internal energy of a gas