Question

If $f$ represents the intermolecular force between molecules and $V$ is the volume occupied by the gas molecules, then at high pressure and at low temperatures, the gas shows large deviation from the ideal behaviour because the fact that

• A. $f$ is negligible
• B. both $f$ and $V$ are negligible
• C. $V$ is negligible
• D. $f$ is appreciable and $V$ is negligible
• E. $f$ is appreciable and $V$ is not negligible

Hint:

Logic Tip: The van der Waals equation $(P + \frac{an^2}{V^2})(V - nb) = nRT$ mathematically corrects for these exact two non-ideal behaviors. The term $\frac{an^2}{V^2}$ corrects for appreciable intermolecular forces ($f$), and $nb$ corrects for non-negligible molecular volume ($V$).

Answer 1

Answer: (E)