Help on 14.11d

[Joanna Pham - 2D]

For 14.11 part d, the question asks us to write the half reactions and the balance redox reaction for the following galvanic cell:

Pt(s) | O2 (g) | H+ (aq) || OH- (aq) | O2 (g) | Pt (g)

I understand that the side to the left of the salt bridge represents oxidation and the side to the right represents reduction, but I have no idea how to write the oxidation and reduction half reactions for this. Could someone help me please?

Thanks!

[Chem_Mod]

H⁺(aq) means there is water in the electrode. Water contains oxygen with a –2 oxidation state. Therefore, the water is being oxidized to O₂(g) (oxidation state of 0). Similarly, in the other electrode, O₂(g) (oxidation state 0) is being reduced to OH^–(aq) (oxidation state –2).