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Using the information from a standard reduction potentials table (see link below), the standard cell potential for the zinc/lead cell is then: EÂºcell = EÂºcathode - EÂºanode = -0.13 - (- 0.76) = 0.63 V.
If the net cell reaction were written in reverse, the cell notation would become. Cu (s) | Cu 2+ (aq) || Zn 2+ (aq) | Zn (s). Remember: the Reduction process is always shown on the Right. 1  The transfer of electrons between an electrode and the solution takes place by quantum-mechanical. 2  at the electrode surface.ositive charge (in the form of Zn 2+) is added to the electrolyte in the left compartment, and removed (as Cu 2+) from the right side, causing the solution in contact with the zinc to acquire a net positive charge, while a net negative charge would build up in the solution on the copper side of the cell.