Question

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.

• A. If both assertion and reason are true and reason is the correct explanation of assertion.
• B. If both assertion and reason are true but reason is not the correct explanation of assertion.
• C. If assertion is true but reason is false.
• D. If both assertion and reason are false.

Answer 1

Answer: (B)

For 1 mole of real gas, $\left(P+\frac{a}{V^{2}}\right)\left(V-b\right)=RT$
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.