[Istafa]

If you have a Zn²⁺/Zn(s) half cell with Zn(s) electrode as the anode with a Fe³⁺/Fe²⁺ half cell with platinum as the electrode the zinc electrode will be anode and the platinum half cell the cathode. But, if you change the platinum electrode to an Fe(s) electrode, what happens?
Right now, i'm thinking that
a) The cell potential changes slightly from that calculated using Eo values as these Eo values use platinum as an inert electrode if no metallic species is present
b) There are no other immediate effects as the Zn(s) is a stronger reductant than Fe(s) and will react at the anode preferentially, so the Fe(s) will not react with Fe³⁺ in solution, even though they are in direct contact
I'm not sure about both of these, however. For b) since they are in direct contact (the solid iron and iron(III) ions) is it that a reaction should occur where iron is oxidised by the Fe³⁺ or not? Would this mean that both reduction and oxidation occurs at the Iron electrode
Fe³⁺(aq)+e^- :rarrow:Fe²⁺ (using electrons from oxidation of zinc at anode)
and the iron electrode also reacting
Fe(s) :rarrow:Fe²⁺(aq)+2e^- (also getting oxidised by Fe³⁺ at the electrode surface?
Thanks for any help in advance!

[Professor 0110]

The zinc electrode will be oxidized, and reduction will take place at the iron electrode. Iron has a higher reduction potential than Zinc. Iron's E value is -0.44 volts, and Zinc's E value is: -0.76. Therefore, zinc is oxidized, and iron is reduced. So more iron will form on the iron electrode.