Redox Reactions

Moderators: Chem_Mod, Chem_Admin

Posts: 21
Joined: Fri Jul 22, 2016 3:00 am
Been upvoted: 1 time

Redox Reactions

Postby Beata_Vayngortin_3L » Wed Feb 01, 2017 8:25 pm

After today's lecture I am still a little unclear on which reaction we need to flip the sign for. I understand that when you have two half reactions you will need to flip one to get the proper sign, but do you always flip the anode or does it depend on the situation?

Jessica Phan 2N
Posts: 15
Joined: Sat Jul 09, 2016 3:00 am

Re: Redox Reactions

Postby Jessica Phan 2N » Wed Feb 01, 2017 9:26 pm

A redox reaction is a chemical reaction involving a reduction and an oxidation. When you are given two half reactions that are shown as reductions, you need to change one to an oxidation reaction, hence one half reaction needs to be reversed. When you reverse the half reaction from a reduction to oxidation, you need to change the sign of E. To find the net potential for the reaction, you will need to add the standard potential for each half reaction, hence you reverse the half reaction that will produce the highest positive E°cell if they are asking for a spontaneous reaction.

On the other hand, when using the formula, E°cell = E°cathode - E°anode, you do not need to flip the sign because it has already taken into account the sign change.

Return to “Balancing Redox Reactions”

Who is online

Users browsing this forum: No registered users and 0 guests