Question 14.11 (d)

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Raymond Le 2G
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Question 14.11 (d)

Postby Raymond Le 2G » Wed Feb 03, 2016 12:26 am

"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)"

How can you tell that O2 reacts with H+ in its respective half-reaction?

Chem_Mod
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Re: Question 14.11 (d)

Postby Chem_Mod » Wed Feb 03, 2016 3:05 am

The half reaction occurs on the same side of the cell so since O2 is in the same side as H+, that is the half reaction. We ignore the platinum electrode because we know that it is an inert electrode and inert electrodes are always positioned in the written formula at the ends.

Laila Sathe 1D
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Re: Question 14.11 (d)

Postby Laila Sathe 1D » Fri Feb 05, 2016 12:41 pm

How do you know what reaction takes place between the O2 and H+? I understand that they react because they are on the same side of the double line in the cell diagram, but I don't get how you figure out what reaction takes place.

Nicholas Wu 3E
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Re: Question 14.11 (d)

Postby Nicholas Wu 3E » Fri Feb 05, 2016 6:04 pm

I believe it is more on the basis of which half reactions you can find an appropriate equation for in the appendix, or whatever is provided - obviously, there are a lot of compounds you can make with just oxygen and hydrogen.


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