Question

You want to “plate out” nickel-metal from a nickel nitrate solution onto a piece of metal inserted into the solution. Should you use copper or zinc (or can you use either)? Explain.

Short answer

The metal used between zinc and copper in the cell shouldbe determined. It’s better to use copper than zinc.

Step-by-step solution

Definition of galvanic cell and its electrodes

The device in which free energy of chemical and physical process can be converted into electrical energy called galvanic cell. These cells contain two electrodes which are immersed in one or more electrolytes.

Plate out the metal

The plating out of any metal named cathode than the other metal as anode. When Zinc combines with the Nickel, it acts as anode between copper and zinc. Since $Z{n}^{2+}/Zn$has a lower standard reduction potential than couple of$N{i}^{2+}/Ni.$

Change to plate out nickel metal from nickel nitrate

Zinc should be oxidized to$Z{n}^{2+}\&N{i}^{2+}$and will reduced to Ni. It’s better to use copper than zinc and changes to plate out nickel metal from nickel nitrate. $Z{n}^{2+}/Zn$has higher standard reduction potential than$N{i}^{2+}/Ni$.