Answer:
[tex]\Delta G_{rxn}=42.7\frac{kJ}{mol}[/tex]
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:
[tex]\Delta G_{rxn}=-RTln(K)[/tex]
But in this case K is just Ka, therefore, at 296 K, it turns out:
[tex]\Delta G_{rxn}=-8.314\frac{J}{mol*K}*296K*ln(2.9x10^{-8})\\\\\Delta G_{rxn}=42.7\frac{kJ}{mol}[/tex]
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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