Balancing redox reactions

Moderators: Chem_Mod, Chem_Admin

Anaranjo
Posts: 14
Joined: Wed Nov 18, 2015 3:00 am

Balancing redox reactions

Postby Anaranjo » Sun Feb 12, 2017 8:39 pm

Balance the following skeletal equations by using oxidation and reduction half-reactions. Identify the oxidizing agent and reducing agent in each reaction.

Mn^2+(aq)+Br2(l)->MnO4^-(aq)+Br(aq)

Chem_Mod
Posts: 18400
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 435 times

Re: Balancing redox reactions

Postby Chem_Mod » Sun Feb 12, 2017 10:59 pm

From page 564-565 of textbook, 6th ed.

1. Write the skeletal equation for both parts:


2. Balance all elements except H and O

3. Balance the O atoms by adding

4. Balance the H atoms by adding

5. Balance the net charges by adding electrons.


Repeat process for Bromine. Figure out which species is gaining electrons (reduction) which species is losing electrons (oxidation). In this case Manganese is being reduced (+7 going to +2 oxidation number)

Sarai_Ferrer_3C
Posts: 14
Joined: Fri Jun 17, 2016 11:28 am

Re: Balancing redox reactions

Postby Sarai_Ferrer_3C » Sun Feb 12, 2017 11:07 pm

Can someone explain to me the reason why we balance reactions under basic conditions differently than when balancing reactions under acidic conditions?

Chem_Mod
Posts: 18400
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 435 times

Re: Balancing redox reactions

Postby Chem_Mod » Sun Feb 12, 2017 11:29 pm

Because in acidic conditions there will be protons available, and in basic conditions there are hydroxy anions. There would be no protons in basic conditions because the base would have absorbed this already.


Return to “Balancing Redox Reactions”

Who is online

Users browsing this forum: No registered users and 1 guest