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First law of thermodynamics, heat capacity

Problem 2.58

One mole of oxygen is expanded from a volume \(V_{1}\) \(=1.00 \mathrm{l}\) to \(V_{2}=5.01\) at a constant temperature \(T=280 \mathrm{~K} .\) Calculate: (a) the increment of the internal energy of the gas: (b) the amount of the absorbed heat. The gas is assumed to be a Van der Waals gas.

Reveal Answer
2.58. (a) \(\Delta U=a / V_{1}-a / V_{2}=0.11 \mathrm{~kJ} ;\) (b) \(Q=R T \ln \frac{V_{2}-b}{V_{1}-b}=\) \(=3.8 \mathrm{~kJ}\)
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