The electromotive force for the cell is Cu_{( | vedclass

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(D) For a concentration cell,the standard cell potential $E_{cell}^{o} = 0$.Using the Nernst equation: $E_{cell} = E_{cell}^{o} - \frac{RT}{nF} \ln \f

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$ - \frac{RT}{F} \ln (0.2) $

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(D) For a concentration cell,the standard cell potential $E_{cell}^{o} = 0$.Using the Nernst equation: $E_{cell} = E_{cell}^{o} - \frac{RT}{nF} \ln \frac{[Cu^{+2}]_{anode}}{[Cu^{+2}]_{cathode}}$Here,$n = 2$,$[Cu^{+2}]_{anode} = 0.004 \ M$,and $[Cu^{+2}]_{cathode} = 0.1 \ M$.Substituting the values: $E_{cell} = 0 - \frac{RT}{2F} \ln \frac{0.004}{0.1}$$E_{cell} = - \frac{RT}{2F} \ln (0.04)$Since $0.04 = (0.2)^{2}$,we have $E_{cell} = - \frac{RT}{2F} \ln (0.2)^{2}$Using the logarithm property $\ln(x^{a}) = a \ln(x)$: $E_{cell} = - \frac{RT}{2F} 	imes 2 \ln (0.2)$$E_{cell} = - \frac{RT}{F} \ln (0.2)$

The electromotive force for the cell is $Cu_{(s)} | Cu_{(0.004 \ M)}^{+2} || Cu_{(0.1 \ M)}^{+2} | Cu_{(s)}$

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