(A) The compressibility factor $Z$ is defined as $Z = \frac{PV_m}{RT}$,where $V_m$ is the molar volume.Rearranging for $V_m$,we get $V_m = \frac{ZRT}{

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(A) The compressibility factor $Z$ is defined as $Z = \frac{PV_m}{RT}$,where $V_m$ is the molar volume.Rearranging for $V_m$,we get $V_m = \frac{ZRT}{P}$.Given values: $Z = 1.5$,$P = 2 \ atm$,$T = 400 \ K$,and $R = 0.08 \ L \ atm \ K^{-1} \ mol^{-1}$.Substituting the values: $V_m = \frac{1.5 \times 0.08 \times 400}{2}$.$V_m = \frac{1.5 \times 32}{2} = 1.5 \times 16 = 24 \ L$.

Class 11 Chemistry States of Matter Real gases and Vander waal’s equation

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$CH_4$ gas is behaving non-ideally. The compressibility factor for the gas is $1.5$ at $2 \ atm$ and $400 \ K$. Calculate the molar volume for the gas in $litre$. [Given $R = 0.08 \ L \ atm \ K^{-1} \ mol^{-1}$]

A
$24$
B
$16$
C
$48$
D
$8$

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States of Matter

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Real gases and Vander waal’s equation

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$CH_4$ gas is behaving non-ideally. The compressibility factor for the gas is $1.5$ at $2 \ atm$ and $400 \ K$. Calculate the molar volume for the gas in $litre$. [Given $R = 0.08 \ L \ atm \ K^{-1} \ mol^{-1}$]

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Under which of the following conditions does a gas deviate from ideal behaviour?
$A$. Low pressure
$B$. High pressure
$C$. Low temperature
$D$. High temperature

Compressibility factor,$Z$,of a gas is given as $Z = \frac{pV}{nRT}$.
$(i)$ What is the value of $Z$ for an ideal gas?
$(ii)$ For a real gas,what will be the effect on the value of $Z$ above Boyle's temperature?