ASSERTION REASON-STATEMENT 1:if two gases have same value of 'b',but different values of 'a',the gas with a larger value of 'a',will occupy less volume under identical conditions. STATEMENT 2: The gas with a larger value of 'a' will have a larger force of intermolecular attraction.

HI student

Statement 1 is true and the statement 2 is the correct explanation for statement 1

(P+n²a/V²)(V-nb)=nRT  -Vanderwaal's equation

P-pressure of the gas

V-volume of the gas

R-gas constant; T- absolute temp.

n²a/V² is the pressure correction due to intermolecular attractions and V-nb represents the available/free volume for the gas.

If two gases have the same values of 'b' that indicates the volume of the two gas molecules or atoms is same.

As the value of 'a ' increases the intermolecular attractions increases. So the Volume term in the vanderwaal's equation mathematically also should be decreased.

Hence Statement 1 is true and the statement 2 is the correct explanation for statement 1