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.

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.

Tardigrade Admin · Accepted Answer

For 1 mole of real gas, (P+(a/V2))(V-b)=RT when V is very large, the terms b and a/v2 are negligible and the van der Waals equation becomes ideal gas equation, PV=RT hence, real gases behave like ideal gas.

Q. 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.

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 not the correct explanation of assertion.

If assertion is true but reason is false.

If both assertion and reason are false.

For 1 mole of real gas, $(P + \frac{a}{V ^{2}}) (V - b) = RT$
when $V$ is very large, the terms $b$ and $a / v^{2}$ are negligible and the van der Waals equation becomes ideal gas equation,
$P V = RT$
hence, real gases behave like ideal gas.

Q. 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.