Use cell notation to describe the galvanic cell where copper(II) ions are reduced to copper metal and zinc metal is oxidized to zinc ions.

In electrochemistry, a Galvanic cellis a kind of electrochemical cell in which the current is produced using a redox reaction. Redox reactions involve oxidation as well as reduction. A galvanic cell consists of two half cells. In the one-half cell, oxidation occurs. This half-cell acts as the anode. In the other half cell, reduction occurs, This half-cell is termed as the cathode. These two half cells work together and constitute an electrochemical cell.

Anode (oxidation): \(\quad {\rm{Zn}}(s) \to {\rm{Z}}{{\rm{n}}^{2 + }}(aq) + 2{{\rm{e}}^ - }\)

Cathode (reduction): \({\rm{C}}{{\rm{u}}^{2 + }}(aq) + 2{{\rm{e}}^ - } \to {\rm{Cu}}(s)\)

Overall: \(\quad {\rm{Zn}}(s) + {\rm{C}}{{\rm{u}}^{2 + }}(aq \to {\rm{Z}}{{\rm{n}}^{2 + }}(aq) + {\rm{Cu}}(s)\)

Using cell notation: \({\mathop{\rm Zn}\nolimits} (s)\left| {{\rm{Z}}{{\rm{n}}^{2 + }}(aq) | |{\rm{C}}{{\rm{u}}^{2 + }}(aq)} \right|{\rm{Cu}}(s).\)