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Question

(B) The compressibility factor $Z$ for a real gas is given by the van der Waals equation. Positive deviation $(Z > 1)$ occurs when the repulsive force

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Molecular volume plays dominant role

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(B) The compressibility factor $Z$ for a real gas is given by the van der Waals equation. Positive deviation $(Z > 1)$ occurs when the repulsive forces or the finite volume of gas molecules become significant. In the van der Waals equation $(P + \frac{an^2}{V^2})(V - nb) = nRT$,the constant $b$ represents the excluded volume of the gas molecules. When the pressure is high,the volume of the gas molecules $(nb)$ becomes significant relative to the total volume $V$,leading to $Z > 1$. Therefore,the molecular volume plays a dominant role in causing positive deviation.

Positive deviation from ideal behaviour is due to the fact that

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