14.17 Help

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Raman Ishwar 1J
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Joined: Fri Sep 25, 2015 3:00 am

14.17 Help

Postby Raman Ishwar 1J » Tue Feb 02, 2016 6:21 pm

Problem 14.17 asks you to write balanced half-reactions for the redox reaction of an acidified solution of potassium permanganate and iron(II) chloride.

For MnO4-, how do you know what the charge on manganese will be on the other side of the half-reaction (once Mn has been reduced)? And what about potassium?

And for Iron(II)'s oxidation, the answer key ignores the chlorine. What happens to the chlorine and why isn't it in the half-reaction? It's also not in the cell diagram that is drawn in the answer key.

Ronald Yang 2F
Posts: 86
Joined: Fri Sep 25, 2015 3:00 am

Re: 14.17 Help

Postby Ronald Yang 2F » Tue Feb 02, 2016 10:19 pm

Usually, when we have MnO4-, it is reduced to Mn2+. That's just a rule of thumb. Potassium is a spectator ion, so I believe that's why we don't take that into account. Similarly, because chlorine is neither oxidized or reduced in this half-reaction, it just acts as a spectator ion, not necessary for half-reactions.

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