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# The reaction which occur in the Galvanic cell is                 (Q). If $\left[{\mathrm{H}}_{3}{\mathrm{O}}^{+}\right]=2.0\mathrm{M},\left[{\mathrm{Fe}}^{3+}\right]=2.0\mathrm{M},\left[{\mathrm{Fe}}^{2+}\right]=0.5\mathrm{M}$ $\left[{\mathrm{Mn}}^{2+}\right]=0.5\mathrm{M},\left[{\mathrm{MnO}}_{4}^{-}\right]=1.0\mathrm{M}$Calculate the emf of the cell.

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a
-0.747 V
b
+0.747 V
c
-0.733
d
+0.736 V
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detailed solution

Correct option is D

Ecell =0.74V−RT5Fln⁡(0.5)(2.0)5(1.0)(2.0)8(0.5)5         =0.74V−0.0595log⁡1(2.0)3(0.5)4         =0.74V−0.0595log⁡2=0.74V−0.059×0.3015=0.736V

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