The Gibbs change (in J) for the given reaction at [Cu2+] = [Sn2+] = 1 M and 298K is : Cu(s) + Sn2+(aq.) $ \to $ Cu2+(aq.) + Sn(s); ($E_{S{n^{2 + }}|Sn}^0 = - 0.16\,V$, $E_{C{u^{2 + }}|Cu}^0 = 0.34\,V$) Take F = 96500 C mol–1)

Question

The Gibbs change (in J) for the given reaction at
[Cu²⁺] = [Sn²⁺] = 1 M and 298K is :

Cu(s) + Sn²⁺(aq.) $ \to $ Cu²⁺(aq.) + Sn(s);

($E_{S{n^{2 + }}|Sn}^0 = - 0.16\,V$,
$E_{C{u^{2 + }}|Cu}^0 = 0.34\,V$)
Take F = 96500 C mol^–1)

Correct Answer

96500

Solution

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