For a reaction,A_{(s)} + 2B_{(aq)}^{+} rightl | vedclass

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Question

(C) The relationship between the standard cell potential $E_{Cell}^{\circ}$ and the equilibrium constant $K_{c}$ is given by the Nernst equation at $2

Vedclass · Accepted Answer

$0.355$

Vedclass · Answer

(C) The relationship between the standard cell potential $E_{Cell}^{\circ}$ and the equilibrium constant $K_{c}$ is given by the Nernst equation at $298 \ K$: $E_{Cell}^{\circ} = \frac{0.0591}{n} \log K_{c}$ Here,the number of electrons transferred $n = 2$. Given $K_{c} = 10^{12}$. Substituting the values: $E_{Cell}^{\circ} = \frac{0.0591}{2} \log(10^{12})$ $E_{Cell}^{\circ} = 0.02955 	imes 12$ $E_{Cell}^{\circ} = 0.3546 \ V \approx 0.355 \ V$ Thus,the correct option is $C$.

For a reaction,$A_{(s)} + 2B_{(aq)}^{+} \rightleftharpoons A_{(aq)}^{2+} + 2B_{(s)}$,$K_{c}$ is $10^{12}$ at $25^{\circ} C$. The $E_{Cell}^{\circ}$ of the corresponding cell is $(F = 96500 \ C \ mol^{-1})$ (in $V$)

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