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(B) Real gases deviate from ideal behavior because they do not follow the assumptions of the Kinetic Molecular Theory,specifically that there are no i

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Low temperature and high pressure

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(B) Real gases deviate from ideal behavior because they do not follow the assumptions of the Kinetic Molecular Theory,specifically that there are no intermolecular forces and that gas molecules have negligible volume.$1$. At high pressure,the volume of gas molecules becomes significant compared to the total volume,and repulsive forces dominate.$2$. At low temperature,the kinetic energy of molecules decreases,making intermolecular attractive forces significant.Therefore,the maximum deviation from ideal gas behavior occurs at $Low 	ext{ } temperature$ and $High 	ext{ } pressure$.

$P \text{ (bar)}$	$\frac{PV}{RT}$
$1$	$1$
$2$	$1$
$3$	$1$
$3.1$	$1.2$
$3.5$	$1.4$
$4.0$	$1.5$

Under which conditions does a real gas show maximum deviation from ideal gas behavior?

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