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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 $High 	ext{ } pressure$.

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

Similar Questions

Which of the following represents the $Van \ der \ Waals$ equation for $n$ moles of a real gas?

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Statement $-2$: The compressibility factor is independent of pressure at the critical temperature.

Under what conditions do real gases behave as ideal gases?

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In the following compressibility factor $(Z)$ versus pressure graph at $300 \, K$,the compressibility of $CH_{4}$ at pressure $< 200 \, bar$ deviates from ideal behaviour because

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