14.5a

[Angela 1K]

Can someone please walk me through how to do this problem?
It's asking to balance the equation O₃(aq) + Br^-(aq) --> O₂(g) + BrO₃^-.
I'm just confused on how to balance this when the atoms being oxidized and reduced are both present in the same molecule in the products.

[Jason Liu 1C]

The atoms being oxidized and reduced actually aren't both present in the same molecule in the products. The oxidation half reaction is O3 --> O2 and the reduction half reaction is Br- --> BrO3-

[Angela 1K]

The atoms being oxidized and reduced actually aren't both present in the same molecule in the products. The oxidation half reaction is O3 --> O2 and the reduction half reaction is Br- --> BrO3-

I don't understand how O₃ is being reduced to O₂ if the oxidation state of both oxygen atoms are 0.

[Leanne Wong 1H]

O₃ is being reduced because you have to balance the half reaction of O₃ -> O₂ which would have H₂O on the O₂ side which would then force there to be two hydrogen ions on the ozone side which means that it would also have 2e- on that side too. Therefore, ozone is reduced since it is gaining electrons.

[Erik Khong 2E]

In my opinion, it's easier to start with the Br part of the question first. It'll end up being the oxidation half of the reaction, and you can just assume that the O3 part will be the reduction half.