The cell,Zn | Zn^{2+} ,(1 M) || Cu^{2+} (1 M) | vedclass

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(D) When the cell is completely discharged,the cell potential $E_{cell} = 0 \ V.$The Nernst equation for the cell reaction is given by:$E_{cell} = E_{

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$10^{37.3}$

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(D) When the cell is completely discharged,the cell potential $E_{cell} = 0 \ V.$The Nernst equation for the cell reaction is given by:$E_{cell} = E_{cell}^{\circ} - \frac{0.059}{n} \log \left( \frac{[Zn^{2+}]}{[Cu^{2+}]} ight)$Here,$n = 2$ (number of electrons transferred) and $E_{cell}^{\circ} = 1.10 \ V.$Substituting the values:$0 = 1.10 - \frac{0.059}{2} \log \left( \frac{[Zn^{2+}]}{[Cu^{2+}]} ight)$Rearranging the equation:$\log \left( \frac{[Zn^{2+}]}{[Cu^{2+}]} ight) = \frac{1.10 	imes 2}{0.059} \approx 37.288 \approx 37.3$Therefore,$\frac{[Zn^{2+}]}{[Cu^{2+}]} = 10^{37.3}$.

The cell,$Zn\ |\ Zn^{2+} \,(1\ M)\ ||\ Cu^{2+}\ (1\ M)\ |\ Cu$ $(E^o_{cell} = 1.10\ V)$ was allowed to be completely discharged at $298\ K.$ The relative concentration of $Zn^{2+}$ to $Cu^{2+}$ $\left( \frac{[Zn^{2+}]}{[Cu^{2+}]} \right)$ is

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