Critical temperature of $N_{2}, C O$ and $C H_{4}$ are $126, 134$ and $190$ K respectively. Arrange them in increasing order of adsorption on the surface of activated charcoal?

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Solution

Adsorption of gas on the surface of activated charcoal depends on the critical temperature of the gas. Critical temperature is that temperature at which or above which the gas cannot be liquefied no matter how much pressure is increased. Critical temperature has a direct relation to adsorption - Higher the critical temperature, greater will be the adsorption.

Gases having higher critical temperature are easily liquefied. Hence in liquid state, they have greater force of attraction with the charcoal and therefore they are more easily adsorbed on the surface of the charcoal. Therefore, the order for adsorption is $N_{2} < C O < C H_{4}$

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Gas	$H_{2}$	$C H_{4}$	$C O_{2}$	$S O_{2}$
Critical Temperature $(K)$	$33$	$190$	$304$	$630$

Gas	$C O_{2}$	$S O_{2}$	$C H_{4}$	$H_{2}$
Critical temp./K	$304$	$630$	$190$	$33$

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