Every real gas behaves as an ideal gas:

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(A) Real gases obey the van der Waals equation:$(P + \frac{n^2 a}{V^2})(V - nb) = nRT$At high temperature $(T)$ and low pressure $(P)$,the volume $V$

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At high temperature and low pressure

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(A) Real gases obey the van der Waals equation:$(P + \frac{n^2 a}{V^2})(V - nb) = nRT$At high temperature $(T)$ and low pressure $(P)$,the volume $V$ becomes very large. Consequently,the correction terms $\frac{n^2 a}{V^2}$ and $nb$ become negligible compared to $P$ and $V$ respectively.Thus,the equation simplifies to $PV = nRT$.Therefore,real gases behave as ideal gases at high temperature and low pressure.

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