Discussion
At high temperature and low density the van der Waals equation should reduce to the ideal gas law. This happens because
Answer: A
Correct answer: both the a and b corrections become negligible
Van der Waals writes \[ \left(P + \frac{a}{V^{2}}\right)(V-b) = RT. \] At low density \( V \) is large, so \( a/V^{2} \) becomes negligible beside \( P \) and \( b \) becomes negligible beside \( V \); at high temperature the attractive term matters less still relative to the thermal energy. With both corrections vanishing the equation collapses to \( PV = RT \) - as any equation of state must in that limit.
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