Writing Balanced Equations for Galvanic Cells (14.11 part d sixth edition)

[KatelinTanjuaquio 1L]

Question 14.11 of the sixth edition, part d states:

Write the half-reactions and the balanced equation for the cell reaction for each of the following galvanic cells. Pt(s) | O2(g) | H+ (aq) || OH-(aq) | O2(g) | Pt(s).

I understand how the anode reaction is derived, but how is the cathode reaction found? Whenever I try, my answer does not match the one in the solutions manual.

[josie 1C]

you have to make sure that you're writing the cathode as a reduction reaction, so the product should have less charge than the reactant

[Kessandra Ng 1K]

To add onto what the user above said, what to remember is that because it's reduction, you add on electrons onto the left side of the equation.

[Charles Hood Disc 1C]

For the cathode, try to imagine the Oxygen as being the electrons supplied to make the OH^-. When it is added to water it will increase the number of electrons and form OH^-. (Really it is the electrons adding on with the oxygen)