The compressibility factor Z = frac{pV}{nRT} | vedclass

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Question

(C) At $NTP$ condition $(p = 1 \ atm, T = 273 \ K)$: For $1 \ mol$ of $H_2$ gas, the molar volume is slightly greater than the ideal gas volume of $22

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greater than one

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(C) At $NTP$ condition $(p = 1 \ atm, T = 273 \ K)$: For $1 \ mol$ of $H_2$ gas, the molar volume is slightly greater than the ideal gas volume of $22.4 \ L \ mol^{-1}$ due to repulsive forces. Using the formula $Z = \frac{pV}{nRT}$, where $R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1}$. For hydrogen gas at $273 \ K$ and $1 \ atm$, the value of $Z$ is approximately $1.0006$. Since $Z > 1$, the compressibility factor for hydrogen gas under these conditions is greater than one.

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 compressibility factor $Z = \frac{pV}{nRT}$ for hydrogen gas at $273 \ K$ and $1 \ atm$ pressure is

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