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The Gibbs energy change (in J) for the given reaction at $$[Cu^{2+}] = [Sn^{2+}] = 1$$ M and 298 K is:
$$Cu(s) + Sn^{2+}(aq.) \to Cu^{2+}(aq.) + Sn(s)$$;
$$(E^0_{Sn^{2+}|Sn} = -0.16 \; V, E^0_{Cu^{2+}|Cu} = 0.34 \; V, \text{Take } F = 96500 \; C \; mol^{-1})$$
Correct Answer: 96500
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