In Appendix D, standard electrode potentials range from about +3 V to -3 V. Thus, it might seem possible to use a halfcell from each end of this range to construct a cell with a voltage of approximately 6 V. However, most commercial aqueous voltaic cells have E° values of 1.5–2 V. Why are there no aqueous cells with significantly higher potentials?

A reaction which occurs in electrochemical process is known as redox reaction. In this chemical reaction, reduction and oxidation of the species take place simultaneously.

When a species releases one electron, it said to undergo oxidation. On the other hand, when a chemical species accepts one electron, it said to undergoes reduction. In electrolytic cell, at cathode reduction takes place where as at anode oxidation take place.

The E° value of a cell can be calculated by subtracting the reduction potential of anode and cathode. The value of reduction potential of a chemical species is calculated in aqueous solution. The chemical species which have high positive value of reduction potential is considered as strong oxidizing agent. On the other hand, the chemical species which have high negative value of reduction potential is strong reducing agent .

When we add strong reducing or oxidizing agent in aqueous solution, it splits water into oxygen and hydrogen gas.

Thus, we concluded that the chemical species which have reduction potential value more than 1.23 V electrolyze water. Therefore, these species cannot used for making commercial aqueous voltaic cell.

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