(C) The compressibility factor is defined as $Z = \frac{V_{real}}{V_{ideal}}$.Since $Z > 1$,it implies that $V_{real} > V_{ideal}$.At $STP$,the molar

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(C) The compressibility factor is defined as $Z = \frac{V_{real}}{V_{ideal}}$.Since $Z > 1$,it implies that $V_{real} > V_{ideal}$.At $STP$,the molar volume of an ideal gas is $V_{ideal} = 22.4 \, dm^3$.Therefore,for a gas with $Z > 1$,the real molar volume $V_m$ must be greater than $22.4 \, dm^3$.

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

Medium

If the compressibility factor $(Z)$ of a gas at $STP$ is greater than $1$,then what will be the value of its molar volume $(V_m)$?

A
Equal to $22.4 \, dm^3$
B
Depends on its molecular size
C
Greater than $22.4 \, dm^3$
D
Less than $22.4 \, dm^3$

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Class 11

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States of Matter

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Real gases and Vander waal’s equation

Excluded volume $(v)$ per molecule is related to the van der Waals constant $'b'$ in the following way:

Medium

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Calculate the compressibility factor $(Z)$ of $1 \text{ mole}$ of a certain real gas if it occupies $0.4 \text{ dm}^3$ at $300 \text{ K}$ and $40 \text{ atm}$. [Given: $R = 0.082 \text{ dm}^3 \text{ atm K}^{-1} \text{ mol}^{-1}$]

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For a non-ideal gas,identify the term in the van der Waals equation that represents the intermolecular forces.

Easy

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For $NH_3$ gas,the $Z$ vs pressure $(P)$ curve at different temperatures is shown. What is the correct order of temperatures? (Given $T_B$ = Boyle temperature)

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Four gases $P, Q, R$ and $S$ have almost same values of $b$ but their $a$ values ($a, b$ are van der Waals' constants) are in the order $Q < R < S < P$. At a particular temperature among the four gases, the most liquefiable one is

EasyWBJEE 2014

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If the compressibility factor $(Z)$ of a gas at $STP$ is greater than $1$,then what will be the value of its molar volume $(V_m)$?

Similar Questions

Excluded volume $(v)$ per molecule is related to the van der Waals constant $'b'$ in the following way:

Calculate the compressibility factor $(Z)$ of $1 \text{ mole}$ of a certain real gas if it occupies $0.4 \text{ dm}^3$ at $300 \text{ K}$ and $40 \text{ atm}$. [Given: $R = 0.082 \text{ dm}^3 \text{ atm K}^{-1} \text{ mol}^{-1}$]

For a non-ideal gas,identify the term in the van der Waals equation that represents the intermolecular forces.

For $NH_3$ gas,the $Z$ vs pressure $(P)$ curve at different temperatures is shown. What is the correct order of temperatures? (Given $T_B$ = Boyle temperature)

Four gases $P, Q, R$ and $S$ have almost same values of $b$ but their $a$ values ($a, b$ are van der Waals' constants) are in the order $Q < R < S < P$. At a particular temperature among the four gases, the most liquefiable one is

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