14.5 (a)

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Lindsay H 2B
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Joined: Fri Sep 29, 2017 7:07 am
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14.5 (a)

Postby Lindsay H 2B » Fri Feb 16, 2018 10:31 am

O3(aq)+Br-(aq) -> O2(g)+BrO3-(aq)
The solutions manual says oxygen is being oxidized from a -2 oxidation state in O3 to a 0 oxidation state in O2. I really don't understand what's going on in this reaction, since both O3 and O2 have neutral charges, and because the solutions manual also shows O3 gaining electrons so I thought that would mean it's getting reduced. Can anyone clear this up?

Danah Albaaj 1I
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Joined: Fri Sep 29, 2017 7:07 am

Re: 14.5 (a)

Postby Danah Albaaj 1I » Fri Feb 16, 2018 1:53 pm

It's really confusing to be asked which is the oxidizing agent and which is the reducing agent. It's the opposite of the reaction the molecule would be in, so O3 is in the reduction reaction which means it is the oxidizing agent.


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