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Liquefaction

Given are the...

Question

Given are the values of their van der Waal's constant 'a'. Arrange the following gases in the order of their expected liquification pressure at a temperature T. T is below the critical point of all the gases.
Gas $C H_{4}$ $K r$ $N_{2}$ $C l_{2}$
'a'( $a t m L^{2} . m o l^{- 1}$ ) 2.283 2.439 1.408 6.579

C H_{4}

K r

N_{2}

C l_{2}

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N_{2}

C H_{4}

K r

C l_{2}

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C l_{2}

K r

C H_{4}

N_{2}

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C l_{2}

N_{2}

K r

C H_{4}

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Solution

The correct option is C $C l_{2}$ < $K r$ < $C H_{4}$ < $N_{2}$
Van der Waals constant 'a' is a indirect measure of attractive force. Gases with higher values of 'a' can be easily liquified. Hence, lower will be its liquefaction pressure.
The increasing order of the van der Waal's constant 'a' is $N_{2} < C H_{4} < K r < C l_{2}$ .
Hence the decreasing order of the liquification pressure is $N_{2} > C H_{4} > K r > C l_{2}$ .

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Similar questions

a

T

T

Gas	$C H_{4}$	$K r$	$N_{2}$	$C l_{2}$
$a (a t m L^{2} . m o l^{- 1})$	2.283	2.439	1.408	6.579

a

\begin{matrix} Gas & a (L^{2} a t m m o l^{- 2}) N_{2} & 1.390 O_{2} & 1.360 N H_{3} & 4.170 C H_{4} & 2.253 \end{matrix}

C H_{4}, N_{2}, N H_{3}

O_{2}

L^{2} a t m m o l^{- 2}

(Z = \frac{P V}{n R T})

O_{2}, N_{2}, N H_{3}

C H_{4}

1.360, 1.390, 4.170

2.253

L^{2}

^{- 2}

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