For the cell Co | Co^{+2} (C_2) || Co^{+2} (C | vedclass

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(B) For a spontaneous reaction,$\Delta G  0$. For the given concentration cell,the cell reaction is $Co^{+2} (C_1) \righ

Vedclass · Accepted Answer

$C_1 > C_2$

Vedclass · Answer

(B) For a spontaneous reaction,$\Delta G  0$. For the given concentration cell,the cell reaction is $Co^{+2} (C_1) \rightarrow Co^{+2} (C_2)$. The Nernst equation for this cell is $E_{cell} = E_{cell}^{\circ} - \frac{0.0591}{n} \log \frac{Q}{K_c}$. Since $E_{cell}^{\circ} = 0$ for a concentration cell,$E_{cell} = -\frac{0.0591}{2} \log \frac{C_2}{C_1} = \frac{0.0591}{2} \log \frac{C_1}{C_2}$. For $E_{cell} > 0$,we must have $\log \frac{C_1}{C_2} > 0$,which means $\frac{C_1}{C_2} > 1$,or $C_1 > C_2$.

For the cell $Co | Co^{+2} (C_2) || Co^{+2} (C_1) | Co$,$\Delta G$ is negative if

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