Keeping in view the values of standard reduction potential given above, which one of the following would you select as a feasible redox chemical reaction?

Explanation

For a redox reaction to be feasible, the emf of it must be positive. (NOTE: When calculating emf, you take the voltage of each half equation according to the scenario, i.e. one will exhibit the same order as those shown above so, the E value is directly taken, but for some, you have to reverse the sign of the E value since the reaction, itself, is reversed). In option A, the emf is = -1.36 + 0.54 = -0.82, so NOT FEASIBLE. In option B, the emf is = -0.34 -0,76 = -1.10, so NOT FEASIBLE. In option C, the emf is = 2.37 + 0.00V = 2.37 so, it IS FEASIBLE; the answer is C. In option D, the emf is = -1.50 + 0 = -1.54 (the coefficient of the reaction is not taken into account) so, it is NOT FEASIBLE.