In a cell,the following reactions take place: | vedclass

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Question

(C) For a spontaneous reaction,the cell potential $E^{\circ}_{Cell}$ must be positive.The reduction half-reactions are:$Fe^{3+} + e^{-} \rightarrow Fe

Vedclass · Accepted Answer

$23$

Vedclass · Answer

(C) For a spontaneous reaction,the cell potential $E^{\circ}_{Cell}$ must be positive.The reduction half-reactions are:$Fe^{3+} + e^{-} ightarrow Fe^{2+}$ $\quad$ $E^{\circ} = 0.77 \, V$ (Cathode)$I_{2} + 2e^{-} ightarrow 2I^{-}$ $\quad$ $E^{\circ} = 0.54 \, V$ (Anode)The spontaneous cell reaction is:$2Fe^{3+} + 2I^{-} ightarrow 2Fe^{2+} + I_{2}$$E^{\circ}_{Cell} = E^{\circ}_{Cathode} - E^{\circ}_{Anode}$$E^{\circ}_{Cell} = 0.77 \, V - 0.54 \, V = 0.23 \, V$Given $E^{\circ}_{Cell} = x 	imes 10^{-2} \, V$,we have:$0.23 = x 	imes 10^{-2}$$x = 23$.

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