The standard e.m.f. of a cell, involving one electron change is found to be 0.591\ V at 25^ . The equilibrium constant of the reaction is ( F = 96,500 - Chemistry MCQ AIEEE 2004 2026 | ExamTest.live

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The standard e.m.f. of a cell, involving one electron change is found to be 0.591 V at 2 5^{\circ} C . The equilibrium constant of the reaction is (F = 96, 500 C mol^{- 1}; R = 8.314 JK^{- 1} mol^{- 1}):

Solution & Step-by-step Explanation

Using the relation lo g K_{e q} = \frac{n E ^{\circ}}{0.0591} at 2 5^{\circ} C . Given n = 1 and E^{\circ} = 0.591 V . lo g K_{e q} = \frac{1 \times 0.591}{0.0591} = 10 . K_{e q} = 1 0^{10} .

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The standard e.m.f. of a cell, involving one electron change is found to be 0.591 V at 2 5^{\circ} C . The equilibrium constant of the reaction is (F = 96, 500 C mol^{- 1}; R = 8.314 JK^{- 1} mol^{- 1}):

1.0 \times 1 0^{1}

1.0 \times 1 0^{30}

1.0 \times 1 0^{10}

1.0 \times 1 0^{5}

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