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(A) Real gases deviate from ideal behavior because of the intermolecular forces and the finite volume of gas molecules. At $high$ $pressure$,the volum

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low temperature and high pressure

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(A) Real gases deviate from ideal behavior because of the intermolecular forces and the finite volume of gas molecules. At $high$ $pressure$,the volume of gas molecules becomes significant compared to the total volume. At $low$ $temperature$,the kinetic energy of molecules decreases,allowing intermolecular forces (van der Waals forces) to become significant. Therefore,a gas deviates most from ideal behavior under conditions of $low$ $temperature$ and $high$ $pressure$.

$A$ gas deviates most from ideal behavior when it is subjected to

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