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(A) The van der Waals equation for $1 \ mol$ of a gas is given by $(p + \frac{a}{V_m^2})(V_m - b) = RT$.At high temperature,the kinetic energy of gas

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$pV_m = RT$

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(A) The van der Waals equation for $1 \ mol$ of a gas is given by $(p + \frac{a}{V_m^2})(V_m - b) = RT$.At high temperature,the kinetic energy of gas molecules is very high,making the effect of intermolecular forces $(a/V_m^2)$ negligible.At low pressure,the volume of the gas $(V_m)$ is very large,making the excluded volume $(b)$ negligible compared to $V_m$.Under these conditions,the equation reduces to $pV_m = RT$,which is the ideal gas equation.

What will the van der Waals equation be at high temperature and low pressure?

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