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\( \boldsymbol{E}^{o} \) value of \( \boldsymbol{N} \boldsymbol{i}^{2+} / \boldsymbol{N} \boldsymbol{i} \) is \( -\mathbf{0 . 2 5} \) V and \( A g^{+} / A g \) is \( +0.80 V . \) If a cell is made by taking the two electrodes what is the feasibility of the reaction?

1. since \( E^{\circ} \) value for the cell will be positive, redox reaction is feasible
2. since \( E^{o} \) value for the cell will be negative, redox reaction is not feasible
3. Ni cannot reduce \( A g^{+} \) to Ag hence reaction is not feasible
4. Ag can reduce \( N i^{2+} \) to Ni hence reaction is feasible

Correct answer: since \( E^{\circ} \) value for the cell will be positive, redox reaction is feasible

Solution

Ag⁺/Ag has the more positive reduction potential, so Ag⁺ is reduced at the cathode and Ni is oxidized at the anode. That gives a positive E°cell, which means the redox reaction is spontaneous (feasible).

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