Determine E° for the half-reaction In³⁺(aq) + 3 e⁻ → In(s).

Question

2In(s) + 6H+(aq) -> 2In^3+(aq) + 3H2(g)

E = +0.32 V (this is not the answer)

Answer 1

From a table of standard reduction potentials, you have....

In³⁺ + 3e- ==> In(s) Eº = -0.34 V (this would be the anode where oxidation takes place)

This would be the Eº for the half reaction. So it is -0.34 V (or -0.32 V if you have a different value from your table). The Eºcell would be +0.32 V (or +0.34 V) if you include the H2/Pt electrode. Not sure what your question is?