ElectrochemistryMedium

Question

For a cell reaction involving a two-electron change, the standard EMF of the cell is found to be 0.295 V at 25°C. The equilibrium constant of the reaction at 25°C will be

Options

A.1 × 1010
B.1 × 10−10
C.29.5 × 10−2
D.2 × 1010

Solution

$E_{cell}^{o} = \frac{0.059}{n}.\log K_{eq} \Rightarrow 0.295 = \frac{0.059}{2}.\log K_{eq}$

$\therefore K_{eq} = 10^{10}$

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