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Mike Matthews 1D
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Joined: Fri Sep 29, 2017 7:04 am


Postby Mike Matthews 1D » Sun Feb 18, 2018 5:16 pm

Could someone please explain to me how to do homework problem 14.11d, "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).
Thank you

Aijun Zhang 1D
Posts: 53
Joined: Tue Oct 10, 2017 7:13 am

Re: 14.11d

Postby Aijun Zhang 1D » Sun Feb 18, 2018 8:11 pm

Pts are just inert electrodes.
The oxygen and H+ ions are on the anode side. Oxidation occurs anode side. So oxygen in the water will be oxidized into oxygen.
2H2O -->4H+ +O2+4e-
On the cathode side, reduction occurs. So O2 is reduced to OH-.

Then we need to balance the number of electrons on both sides. Since there are 4e- on both sides, we just need to add them up and subtract the same substance.
Then the balanced equation will be : H2O --> H^+ + OH^-

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