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(D) The behavior of a real gas is described by the van der Waals equation: $(P + \frac{a}{V^2})(V - b) = RT$.$1$. At high temperature $(T)$,the averag

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pressure is low and temperature is high

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(D) The behavior of a real gas is described by the van der Waals equation: $(P + \frac{a}{V^2})(V - b) = RT$.$1$. At high temperature $(T)$,the average kinetic energy of the gas molecules is very high,which allows them to overcome the intermolecular forces $(IMF)$.$2$. At low pressure $(P)$,the volume occupied by the gas is large,meaning the molecules are far apart,making the volume of the molecules $(b)$ negligible compared to the total volume and minimizing the effect of intermolecular forces.$3$. Therefore,a real gas approaches ideal gas behavior under the conditions of low pressure and high temperature.

$A$ real gas behaves like an ideal gas if its

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