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14.11 (d)

Posted: Sat Feb 17, 2018 11:42 pm
by Andy Liao 1B
Problem:
14.11 Write the half-reactions and the balanced equation for the cell reaction for each of the following galvanic cells:
(d) Pt(s) | O2(g) | H+(aq) || OH-(aq) | O2(g) | Pt(s)

I was wondering how the solutions manual found the cathode and anode half-reactions for the cell reaction. The cathode is 2H2O(l) + O2(g) + 4e- -> 4OH-(aq) and the anode is O2(g) + 4H+(aq) + 4e- -> 2H2O(l). Can someone please explain?

Re: 14.11 (d)

Posted: Sun Feb 18, 2018 3:48 pm
by 404995677
Hi I found the explanation from another post!

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