If a piece of silver is placed in a solution in which [Ag+] = [Fe2+] = 1.00 M at STP, what is Ecell for the following reaction?

Question

2Ag(s) + Fe²⁺ (aq) --> 2Ag⁺(aq) + Fe(s)

The standard reduction potentials for the species in the reaction above are listed below:

Ag⁺(aq) + e^- --> Ag(s) E(red) = .7996 V

Fe²⁺ (aq) + 2e^- ---> Fe(s) E(red) = -.447 V

Answer 1

Ag⁺(aq) + e^- --> Ag(s) E(red) = .7996 V

Fe²⁺ (aq) + 2e^- ---> Fe(s) E(red) = -.447 V

2Ag(s) + Fe²⁺ (aq) --> 2Ag⁺(aq) + Fe(s)

This has Fe²⁺ being reduced to Fe(s) which would take place at the CATHODE

This has Ag(s) being oxidized to Ag⁺(aq) which would take place at the ANODE

The Ecell = E(cathode) - E(anode)

Ecell = -0.447 - 0.7996

Ecell = -1.25 V (this would be non-spontaneous)

The reaction should be:

2Ag⁺(aq) + Fe(s) ==> 2Ag(s) + Fe²⁺(aq) and then Ecell = +1.25 V (spontaneous)