This is not a homework question but I've been trying to figure this out for hours.

A galvanic cell is prepared by adding a 0.9 M Fe2+ (aq) solution at 298 K to the compartment on the left with an iron (Fe) electrode, as depicted in picrel.
The compartment on the right contains an aqueous solution of 0.9 M H3O+ at 298 K and 1 atm H2 (g) that is bubbled into solution through a Pt electrode.

What the fuck is the overall balanced chemical reaction that would spontaneously occur immediately after the Fe2+ solution is added to the left compartment?
What if you have both Fe3+ (aq) and Fe2+ (aq)?

I'll post the answer after you guys guess and get it wrong.

Note that the reduction potentials (V) are:
Fe 3+ + e- --> Fe 2+
>+0.77
2H3O+ + 2e- --> H2 + 2H2O
>0.00
Fe 2+ + 2e- --> Fe (s)
>-0.45