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(D) real gas obeys the van der Waals equation:$(P + \frac{an^2}{V^2})(V - nb) = nRT$At high temperature,the kinetic energy of gas molecules is very la

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pressure is low and temperature is high

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(D) real gas obeys the van der Waals equation:$(P + \frac{an^2}{V^2})(V - nb) = nRT$At high temperature,the kinetic energy of gas molecules is very large,making the intermolecular forces of attraction negligible.At low pressure,the volume of the gas is very large,making the volume occupied by the gas molecules $(nb)$ negligible compared to the total volume $(V)$.Under these conditions (high temperature and low pressure),the van der Waals equation simplifies to the ideal gas equation: $PV = nRT$.Therefore,a real gas behaves like an ideal gas at low pressure and high temperature.

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

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