Assertion : The gases show ideal behaviour when the volume occupied is large so that the volume of the molecules can be neglected in comparison to it .Reason : The behaviour of the gas becomes more ideal when pressure is very low .

Assertion : The gases show ideal behaviour when the volume occupied is

1.	Assertion : The gases show ideal behaviour when the volume occupied is large so that the volume of the molecules can be neglected in comparison to it .Reason : The behaviour of the gas becomes more ideal when pressure is very low .
Answer» If both ASSERTION and reason are TRUE and reason is the correct explanation of assertion . If both assertion and reason are true but reason is NOTTHE correct explanation of assertion . If assertion is true but reason is false . If both assertion and reason are false . Solution :For 1 mole of real gas, `(P+(a)/(V^(2)))(V-b)=RT` when V is very large, the terms b and `a//V^(2)` are negligible and the van der Waals equation becomes ideal gas equation, PV = RT hence, real gases behave like ideal gas.