[Four-digit Integer] One mole of a van der Waals gas expands reversibly and isothermally at 27°C from 2 L to 20 L. The magnitude of work done (in J) if a = 1.42 × 10^12 dynes cm^4/mol and b = 30 ml/mo

Question

[Four-digit Integer] One mole of a van der Waals gas expands reversibly and isothermally at 27°C from 2 L to 20 L. The magnitude of work done (in J) if a = 1.42 × 10^12 dynes cm^4/mol and b = 30 ml/mol.

Prashant Kotian · Accepted Answer

Correct answer: 5778. Work = nRT ln[(V2-nb)/(V1-nb)] + a/n × (1/V1 - 1/V2). Numerical integration gives 5778 J.

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