A van der Waals' gas may behave ideally when | vedclass

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(C) The van der Waals' equation for $n$ moles of a gas is $(P + \frac{an^2}{V^2})(V - nb) = nRT$. At very low pressure, the volume $V$ is very large,

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the pressure is very low

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(C) The van der Waals' equation for $n$ moles of a gas is $(P + \frac{an^2}{V^2})(V - nb) = nRT$. At very low pressure, the volume $V$ is very large, making the term $\frac{a}{V^2}$ negligible. Also, the volume $V$ is much larger than the excluded volume $b$, so $(V - b) \approx V$. Thus, the equation reduces to $PV = RT$, which is the ideal gas equation. Therefore, a van der Waals' gas behaves ideally at very low pressure.

$A$ van der Waals' gas may behave ideally when

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