Have I done it correctly?

Question

Hi!

I need to know I am thinking correctly in this question, thanks in advance :)

Does this following reaction occur spontaneously?

Fe³⁺ + Ag(s) + Cl^- --> Fe²⁺ + AgCl (s)

I found that Fe^{2+ ---->} Fe³⁺ + e- Eº = 0.77

But this reaction goes Fe³⁺ + e- ---->Fe²⁺ so the Eº = -0.77

Then I have Ag⁺ + e- ----> Ag(s) Eº = +0.80 V

The difference is= Ereduction-Eoxidation= -0.77-0.80= -1.57

Negative value means nope, it is not spontaneous

Answer 1

First, let's recognize that the Cl- is merely a spectator ion, and has no bearing on the overall reaction.

I think we've discussed this very problem previously, but I'll give you my input again, for what it's worth.

Using the figures you provide, reduction of Fe3+ is 0.77 and reduction of Ag+ is 0.80. This suggests that Ag+ would be reduced and since Ag+ is on the PRODUCT side of the reaction AS WRITTEN, it would not be spontaneous. The spontaneous reaction would be Ag⁺ + Fe²⁺(s) ==> Ag(s) + Fe³⁺

Does this make sense. Also, didn't you and I discuss this in the past? If so, what seems to be the issue now? Just curious.