6th edition 14.5a

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Julia Lung 1I
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Joined: Fri Jun 23, 2017 11:39 am

6th edition 14.5a

Postby Julia Lung 1I » Sun Feb 24, 2019 3:23 pm

The problem asks you to balance the reaction using redox half rxns: O3 + Br- ----> O2 + BrO3-
For this problem O3 is oxidized = 0 to O2 which is -2, I thought O2 is suppose to equal 0 can anyone explain why and in what situations O2 would equal 0 or -2?

Adrian C 1D
Posts: 60
Joined: Fri Sep 28, 2018 12:19 am

Re: 6th edition 14.5a

Postby Adrian C 1D » Sun Feb 24, 2019 3:35 pm

O3 on the reactant side is 0 while it goes to -2 on the product side in BO3-, which makes it the oxidizing agent. Br- goes from -1 on the reactant side to +5 in BrO3- on the product side. O3 and O2 are not the same species. O2 still has 0 oxidation number. Otherwise, oxygen usually is -2. Exceptions are H202 and F2O. In H2O2, it is -1. IN F2O, since oxygen is not the most electronegative-its oxidation number is +2.

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