Question

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.

Short answer

The cell notation is $\mathrm{Zn}(s)\left|\mathrm{Z}{\mathrm{n}}^{2+}(aq)||\mathrm{C}{\mathrm{u}}^{2+}(aq)\right|\mathrm{C}\mathrm{u}(s).$

Step-by-step solution

Define the balanced chemical reactions

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.

Determine the Balance equation

Anode (oxidation): $\mathrm{Z}\mathrm{n}(s)\to \mathrm{Z}{\mathrm{n}}^{2+}(aq)+2{\mathrm{e}}^{-}$

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

Overall: $\mathrm{Z}\mathrm{n}(s)+\mathrm{C}{\mathrm{u}}^{2+}(aq\to \mathrm{Z}{\mathrm{n}}^{2+}(aq)+\mathrm{C}\mathrm{u}(s)$

Using cell notation: $\mathrm{Zn}(s)\left|\mathrm{Z}{\mathrm{n}}^{2+}(aq)||\mathrm{C}{\mathrm{u}}^{2+}(aq)\right|\mathrm{C}\mathrm{u}(s).$