14.13 d

[sofiakavanaugh]

Write the 1/2 rxn, balanced equation, calculate E cell and write the cell diagram for the chemical rxn: Au+(aq) --> Au(s) + Au3+

I got this for the cell diagram: Pt(s)| Au+(aq), Au 3+(aq) || 2Au+(aq) | 2Au(s)

Can someone please explain to me why this is wrong and how to get the correct diagram?

Thanks!

[Hubert Tang-1H]

We split the reaction into the anode and cathode reactions:
Anode: Au(s)--->Au3+ (aq) + 3e-
Cathode: Au+(aq)+e- ----> Au(s)

We see that both the anode and cathode have solid Au, so there shouldn't be Pt in the cell diagram.

Thus, from our anode and cathode, our cell diagram should be

Au(s)| Au3+(aq)||Au+(aq)|Au(s)

[Angela 1K]

How are we supposed to know that the oxidation reaction is Au³⁺(aq) + 3e^- --> Au(s) if, in the reaction given Au and Au³⁺ are on the same side (products)?