Question

Calculate the value of ΔG∘rxnΔGrxn∘ for the following reaction at 296 K. Ka = 2.9 × 10–8 and assume Ka does not change significantly with temperature. $$HClO(aq)+H2O(l) HClO−(aq)+H3O+(aq)

Answer 1

`\Delta G_(rxn)=42.7(kJ)/(mol)`

Step-by-step explanation:

In this case, for the dissociation of hypochlorous acid, we know that the acid dissociation constant (Ka) is 2.9x10⁻⁸, which is related with the Gibbs free energy as shown below:

`\Delta G_(rxn)=-RTln(K)`

But in this case K is just Ka, therefore, at 296 K, it turns out:

`\Delta G_(rxn)=-8.314(J)/(mol*K)*296K*ln(2.9x10^(-8))\\\\\Delta G_(rxn)=42.7(kJ)/(mol)`

Such result, means that the reaction is nonspontaneous at the given temperature, it means it is not favorable (not easily occurring).

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