If a cell has a standard electrode potential | vedclass

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(A) The relationship between standard cell potential $(E^{\circ}_{cell})$ and equilibrium constant $(K_{C})$ is given by the Nernst equation at $298 \

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$1.0 	imes 10^{10}$

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(A) The relationship between standard cell potential $(E^{\circ}_{cell})$ and equilibrium constant $(K_{C})$ is given by the Nernst equation at $298 \ K$: $E^{\circ}_{cell} = \frac{0.0591}{n} \log K_{C}$ Given: $E^{\circ}_{cell} = 0.295 \ V$ and $n = 2$. Substituting the values: $0.295 = \frac{0.0591}{2} \log K_{C}$ $0.295 = 0.02955 \log K_{C}$ $\log K_{C} = \frac{0.295}{0.02955} \approx 10$ $K_{C} = 10^{10} = 1.0 	imes 10^{10}$

If a cell has a standard electrode potential of $0.295 \ V$ and $n = 2$,calculate its equilibrium constant at $298 \ K$.

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