Assertion: Gases like `N_(2), O_(2)` behave as ideal gases at high temperature and low pressure.
Reason: Molecular interaction diminihes at high temperature and low pressure.

At high temperature and low pressure van der Waal's equation becomes

At high temperature and low pressure van der Waal's equation becomes

Statement-1: Gases like N_(2),O_(2) behave as ideal gases at high temperature and low pressure. Statement-2: Molecular probable velocity is the velocity possessed by maximum fraction of molecules at the same temperature. Statement-2:Molecular interactions diminish at high temperature and low pressure.

Why does a real gas behave like an ideal gas at very high temperature and low pressures?

At high temperature and low pressure the van der Waals equation is reduced to .

(A): A gas behaves as an ideal gas at high temperature and low pressure. (R): Helium behaves as an ideal gas under all conditions.

Real gases behave ideally at low temperature and high pressure. b) Justify.

A: A real gas will approach ideal behaviour at high temperature and low pressure. R: At low pressure and high temperature z = 1, for all gases

A: A real gas will approach ideal behaviour at high temperature and low pressure. R: At low pressure and high temperature z = 1, for all gases