For ideal gases, `Z = 1` at all temperature and pressure.

STATEMENT-1 : 1 mol of H_(2) and O_(2) each occupy 22.7 L of volume at 0^(@)C and 1 bar pressure, considering ideal behaviour. STATEMENT-2 : Molar volume for all ideal gases at the same temperature and pressure are equal.

STATEMENT-1 : 1 mol of H_(2) and O_(2) each occupy 22.7 L of volume at 0^(@)C and 1 bar pressure, considering ideal behaviour. STATEMENT-2 : Molar volume for all ideal gases at the same temperature and pressure are equal.

STATEMENT-1 : 1 mol of H_(2) and O_(2) each occupy 22.7 L of volume at 0^(@)C and 1 bar pressure, considering ideal behaviour. STATEMENT-2 : Molar volume for all ideal gases at the same temperature and pressure are equal.

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.

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.

Assertion : Compressibility factor (Z) is the ratio of actual molar volume of a gas to the molar volume of it , if it were an ideal gas at that temperature and pressure . Reason : At high pressure all the gases have Z lt 1 and can be easily compressed .

Molar gas constant is the same for all gases because at the same temperature and pressure, equal volumes of all gases have the same