6L 5C (7th Edition)

[Iona Pay]

The question reads as follows:

Write the half reactions, balanced equation, and cell diagram.

D. Au+(s) ----> Au(s) + Au3+(aq)

The solution manual writes the cell as follows: Au | Au3+ || Au+| Au+.

I'm confused as to why we are allowed to use Au for each electrode, even though only one of the redox reactions has Au as a product or reactant? Why wouldn't this interfere with the galvanic cell?

[Chem_Mod]

The solutions manual could technically choose any metal for the Au+ being oxidized to Au+3 reaction. They probably just decided to use Au since it's a metal that conducts electricity. But they could've used Pt or any other metal that conducts electricity. :)