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}^\circ_{{Sn}^{2+}| {Sn}} =-0.16 {V}, {E}^\circ_{ {Cu}^{2+}| {Cu}} =0.34 {V} ,Take {F}=96500 {C} {\mol}^{-1 }) [2 Sep 2020 Shift 1]

Electrochemistry Part 1

Section: Chemistry

Question : 32 of 100

Marks: +1, -0

The Gibbs energy change (in J ) for the given reaction at [Cu2+]=[Sn2+]=1M and 298 K is:
Cu(s)+Sn2+(aq.)→Cu2+(aq.) +Sn(s)
(E°Sn2+|Sn=−0.16V, E°Cu2+|Cu=0.34V,Take F=96500C mol−1)

[2 Sep 2020 Shift 1]

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