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Chemistry · Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions

value of is V and is If a cell is made by taking the two electrodes what is the

\( \boldsymbol{E}^{o} \) 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?

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

Step-by-step solution

The cell reaction is Ni + 2Ag⁺ → Ni²⁺ + 2Ag. Standard cell potential E°cell = E°cathode (Ag⁺/Ag) - E°anode (Ni²⁺/Ni) = 0.80 V - (-0.25 V) = +1.05 V. A positive E°cell indicates the redox reaction is spontaneous and feasible.
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