## HW 6K.5 a

Hannah Lee 2F
Posts: 117
Joined: Thu Jul 11, 2019 12:15 am

### HW 6K.5 a

Balance each of the following skeletal equations by using oxidation and reduction half-reactions. All the reactions take place in basic solution. Identify the oxidizing agent and reducing agent in each reaction.
Reaction of ozone with bromide ions:
O3(aq) + Br-(aq) --> O2(g) + BrO3-(aq)

I'm confused as to why O3 --> O2 is written as the reduction half-reaction even though the oxidation number isn't changing. Why wouldn't O3 be reduced to BrO3-, since the oxidation # changes from 0 to 2- in that case? Also, is there a reason why O3 is written as aqueous state in the balanced reaction in the solutions manual although it is gaseous in the given chemical equation?

Michelle Song 1I
Posts: 102
Joined: Thu Jul 11, 2019 12:17 am

### Re: HW 6K.5 a

My guess for some of your questions would be since Br is being oxidized, you can assume that O3 is reduced, which kinda makes sense considering it loses an oxygen.