Consider the following equilibria for gases : (g) (aq) + 4.6 Kcal ; (g) (aq) + 8.6 Kcal. Assuming the randomness factor to be about the same for each, which of the gases will have the lower solubility

Question

Consider the following equilibria for gases : $H_2S$(g) $H_2S$(aq) + 4.6 Kcal ; $SO_2$(g) $SO_2$(aq) + 8.6 Kcal. Assuming the randomness factor to be about the same for each, which of the gases will have the lower solubility in water ?

Prashant Kotian · Accepted Answer

Correct answer: A. Since, less heat is released in 1st reaction as compared to the heat released in the 2nd reaction. So, 1st reaction is less spontaneous and hence, 2 H S will be less soluble in in water.

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