Under which conditions does the van der Waa | vedclass

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(C) The $van \ der \ Waals$ equation for $n$ moles of a gas is given by: $(P + \frac{an^2}{V^2})(V - nb) = nRT$. For $1$ mole of gas,it is $(P + \frac

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Low pressure and high temperature

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(C) The $van \ der \ Waals$ equation for $n$ moles of a gas is given by: $(P + \frac{an^2}{V^2})(V - nb) = nRT$. For $1$ mole of gas,it is $(P + \frac{a}{V_m^2})(V_m - b) = RT$. At low pressure,the volume $V_m$ is very large,so $b$ becomes negligible compared to $V_m$. At high temperature,the pressure $P$ is significant compared to the internal pressure term $\frac{a}{V_m^2}$,making $\frac{a}{V_m^2}$ negligible. Thus,the equation reduces to $PV_m = RT$,which is the ideal gas equation.

Under which conditions does the $van \ der \ Waals$ equation reduce to the ideal gas equation?

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