Given the critical temperatures () of four gases: , , , and . If precisely of activated charcoal is introduced to an equimolar mixture of these gases, which gas will be most aggressively and heavily p

Question

Given the critical temperatures ($T_c$) of four gases: $H_2 	ext{ (33 K)}$, $N_2 	ext{ (126 K)}$, $CH_4 	ext{ (190 K)}$, and $SO_2 	ext{ (430 K)}$. If precisely $1	ext{ g}$ of activated charcoal is introduced to an equimolar mixture of these gases, which gas will be most aggressively and heavily physically adsorbed?

Prashant Kotian · Accepted Answer

Correct answer: D. Physical adsorption relies directly on universal van der Waals forces. The magnitude of these forces is strictly proportional to the ease of liquefaction, which is measured by the gas's Critical Temperature (). possesses the highest , meaning it has the strongest intermolecular forces and is most heavily adsorbed.

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