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(B) The compressibility factor $(Z)$ is defined as $Z = \frac{PV_m}{RT}$.For an ideal gas, $Z = 1$ at all pressures, which corresponds to the horizont

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Ideal Gas, $H_2, CO_2$

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(B) The compressibility factor $(Z)$ is defined as $Z = \frac{PV_m}{RT}$.For an ideal gas, $Z = 1$ at all pressures, which corresponds to the horizontal line $(A)$.Real gases show deviations from ideal behavior.For gases like $H_2$ and $He$, the intermolecular forces are weak, and the volume effect dominates, leading to $Z > 1$ at all pressures, as shown by curve $(B)$.For easily liquefiable gases like $CO_2$, the attractive forces dominate at low pressures $(Z  1)$, resulting in the characteristic dip shown by curve $(C)$.Therefore, $(A)$ is an ideal gas, $(B)$ is $H_2$, and $(C)$ is $CO_2$.

Gas	$Ar$	$Ne$	$Kr$	$Xe$
$a \ (atm \ dm^6 \ mol^{-2})$	$1.3$	$0.2$	$5.1$	$4.1$
$b \ (10^{-2} \ dm^3 \ mol^{-1})$	$3.2$	$1.7$	$1.0$	$5.0$

The variation of the compressibility factor $(Z)$ with pressure $(P$ in $bar)$ for some gases is shown in the figure below. Identify the gases $(A)$, $(B)$, and $(C)$.

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