## multiplying half reactions [ENDORSED]

davidryan3f
Posts: 63
Joined: Fri Sep 28, 2018 12:23 am

### multiplying half reactions

If you multiply a half reaction by a certain number in order to make the two half reactions have the same number of electrons, do you multiply the cell potential for the half reaction by that same factor?

Chem_Mod
Posts: 18400
Joined: Thu Aug 04, 2011 1:53 pm
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### Re: multiplying half reactions

You would not multiply the cell potential by that same factor. So for example, Ag+1 + e- -> Ag has a standard E value of 0.8 V.

If I were to multiply it by 3, giving me 3Ag+1 + 3e- -> 3Ag, this reaction would also have a standard E value of 0.8 V.

Hope this helps! :)

Destiny Diaz 4D
Posts: 51
Joined: Fri Sep 28, 2018 12:28 am

### Re: multiplying half reactions  [ENDORSED]

I think the only case you would multiply it by something is when you want to flip the reaction so you would multiply the cell potential by negative 1.

Rehan Chinoy 1K
Posts: 67
Joined: Fri Sep 28, 2018 12:25 am

### Re: multiplying half reactions

Yes, if you want a reaction to be the oxidation reaction you flip the sign of the associated cell potential found in the standard reduction potentials table. Otherwise, you never mess with the given cell potential.

dgerges 4H
Posts: 65
Joined: Fri Sep 28, 2018 12:24 am

### Re: multiplying half reactions

you don't multiply cell potential, only the coefficients in the half reaction