Identify the wrong relation for real gases :

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Question

(A) The wrong relation for real gases is given in option $A$. The compressibility factor $Z$ is defined as the ratio of the molar volume of a real gas

Vedclass · Accepted Answer

$Z = \frac{V_{ideal}}{V_{real}}$

Vedclass · Answer

(A) The wrong relation for real gases is given in option $A$. The compressibility factor $Z$ is defined as the ratio of the molar volume of a real gas to the molar volume of an ideal gas at the same temperature and pressure. Therefore,the correct form is $Z = \frac{V_{real}}{V_{ideal}}$. Option $B$ represents the pressure correction term in the van der Waals equation. Option $C$ represents the volume correction term where $V_{real} = V_{ideal} + nb$ is generally used for the excluded volume correction,but in the context of the van der Waals equation $(p + \frac{an^2}{V^2})(V - nb) = nRT$,the relation $V_{real} = V_{ideal} + nb$ is standard. Option $D$ is the van der Waals equation for $1 	ext{ mole}$ of gas.

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

Similar Questions

Which statement is correct regarding a real gas?

$1 \ mol$ of a real gas is kept at a high pressure of $100 \ bar$ at $300 \ K$. If the van der Waals constant $b$ is $0.005 \ L \ mol^{-1}$, what are the values of the compressibility factor $Z$ of the gas and the $\%$ deviation of volume from ideality?
$Z$ $\%$ Deviation

The pressure of real gases is less than that of ideal gas because of:

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 unit of the van der Waals gas equation parameter $a$ in $(P + \frac{an^{2}}{V^{2}})(V - nb) = nRT$ is :

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