HW 14.5

Moderators: Chem_Mod, Chem_Admin

Drishti_Jain_1D
Posts: 22
Joined: Fri Jul 22, 2016 3:00 am

HW 14.5

Postby Drishti_Jain_1D » Tue Feb 14, 2017 7:53 pm

Can someone please explain why the half reaction for oxidation of the reaction in this problem is O3 --> O2 when both the oxidation charges of these molecules are 0? Doesn't oxidation need to have a loss of electrons from the reactant to product?

Chem_Mod
Posts: 18885
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 716 times

Re: HW 14.5

Postby Chem_Mod » Tue Feb 14, 2017 10:23 pm

one O in the O3 gains electron and goes to BrO3-

404639305
Posts: 15
Joined: Fri Sep 25, 2015 3:00 am

Re: HW 14.5

Postby 404639305 » Tue Feb 14, 2017 10:56 pm

yes, so because it is not balanced, you would have to balance it first. It would be: H+ + O3 -> O2 + H2O, which is a reduction half reaction.


Return to “Balancing Redox Reactions”

Who is online

Users browsing this forum: No registered users and 1 guest