(B) The compressibility factor is defined as $Z = \frac{PV_m}{RT}$.For an ideal gas,$Z = 1$ and $V_m = 22.4 \ L$ at $NTP$.If $Z > 1$,the gas shows pos

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(B) The compressibility factor is defined as $Z = \frac{PV_m}{RT}$.For an ideal gas,$Z = 1$ and $V_m = 22.4 \ L$ at $NTP$.If $Z > 1$,the gas shows positive deviation from ideal behavior,meaning the repulsive forces are dominant.Consequently,the molar volume $V_m$ is greater than the ideal molar volume,i.e.,$V_m > 22.4 \ L$ at $NTP$.

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

Medium

If the compressibility factor $(Z)$ is greater than unity,then which of the following is true for the molar volume $(V_m)$ of a gas at $NTP$?

A
$V_m = 22.4 \ L \ (at \ NTP)$
B
$V_m > 22.4 \ L \ (at \ NTP)$
C
$V_m < 22.4 \ L \ (at \ NTP)$
D
$V_m = 11.2 \ L \ (at \ NTP)$

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States of Matter

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Real gases and Vander waal’s equation

The units of constant $a$ in the Van der Waals equation are:

Easy

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$A$ gas at $350 \; K$ and $15 \; bar$ has a molar volume $20$ percent smaller than that for an ideal gas under the same conditions. The correct option about the gas and its compressibility factor $(Z)$ is

MediumNEET 2019

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Consider the van der Waals constants,$a$ and $b,$ for the following gases.

Gas $Ar$ $Ne$ $Kr$ $Xe$

$a \ (atm \ dm^6 \ mol^{-2})$ $1.3$ $0.2$ $5.1$ $4.1$

$b \ (10^{-2} \ dm^3 \ mol^{-1})$ $3.2$ $1.7$ $1.0$ $5.0$

Which gas is expected to have the highest critical temperature?

MediumJEE MAIN 2019

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Explain the compressibility factor $(Z)$.

Medium

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The $Z$ vs $P$ graph for four gases is given below at the same temperature.
Which of the gases will have the highest value of critical temperature $(T_c)$?

Medium

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

If the compressibility factor $(Z)$ is greater than unity,then which of the following is true for the molar volume $(V_m)$ of a gas at $NTP$?

Similar Questions

The units of constant $a$ in the Van der Waals equation are:

$A$ gas at $350 \; K$ and $15 \; bar$ has a molar volume $20$ percent smaller than that for an ideal gas under the same conditions. The correct option about the gas and its compressibility factor $(Z)$ is

Consider the van der Waals constants,$a$ and $b,$ for the following gases. Gas $Ar$ $Ne$ $Kr$ $Xe$ $a \ (atm \ dm^6 \ mol^{-2})$ $1.3$ $0.2$ $5.1$ $4.1$ $b \ (10^{-2} \ dm^3 \ mol^{-1})$ $3.2$ $1.7$ $1.0$ $5.0$ Which gas is expected to have the highest critical temperature?

Explain the compressibility factor $(Z)$.

The $Z$ vs $P$ graph for four gases is given below at the same temperature.Which of the gases will have the highest value of critical temperature $(T_c)$?

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Consider the van der Waals constants,$a$ and $b,$ for the following gases.

Gas $Ar$ $Ne$ $Kr$ $Xe$

$a \ (atm \ dm^6 \ mol^{-2})$ $1.3$ $0.2$ $5.1$ $4.1$

$b \ (10^{-2} \ dm^3 \ mol^{-1})$ $3.2$ $1.7$ $1.0$ $5.0$

Which gas is expected to have the highest critical temperature?

The $Z$ vs $P$ graph for four gases is given below at the same temperature.
Which of the gases will have the highest value of critical temperature $(T_c)$?