For a gas,the deviation from ideal behavior i | vedclass

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(D) Real gases deviate from ideal behavior under conditions of high pressure and low temperature.This is because at low temperatures,the kinetic energ

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$-13\,^oC$ and $2.0\, atm$

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(D) Real gases deviate from ideal behavior under conditions of high pressure and low temperature.This is because at low temperatures,the kinetic energy of gas molecules decreases,making intermolecular forces significant.At high pressures,the volume occupied by the gas molecules becomes significant compared to the total volume of the container.Comparing the given options,the condition with the lowest temperature and highest pressure will show the maximum deviation.Comparing $-13\,^oC$ and $2.0\, atm$ with other options,it is the lowest temperature and highest pressure combination.Therefore,the deviation is maximum at $-13\,^oC$ and $2.0\, atm$.

For a gas,the deviation from ideal behavior is maximum at:

Similar Questions

For $1 \ mol$ of $CO_2$ gas at $300 \ K$ temperature and $40 \ atm$ pressure occupying a volume of $0.4 \ L$,the compressibility factor $Z$ indicates that the gas is:

Which gas shows real behavior?

The given graph represents the variation of $Z$ (compressibility factor = $\frac{PV}{nRT}$) versus $P$,for three real gases $A, B$ and $C$. Identify the only incorrect statement.

Statement $-1$: The compressibility factor at the critical point is the same for different gases following van der Waal's equation.
Statement $-2$: The compressibility factor is independent of pressure at the critical temperature.

One of the assumptions of the kinetic theory of gases is that there is no force of attraction between the molecules of a gas. State and explain the evidence that shows that this assumption is not applicable for real gases.

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