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multiplying half reactions

Posted: Sat Mar 16, 2019 3:29 pm
by davidryan3f
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?

Re: multiplying half reactions

Posted: Sat Mar 16, 2019 3:50 pm
by Chem_Mod
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! :)

Re: multiplying half reactions  [ENDORSED]

Posted: Sat Mar 16, 2019 4:18 pm
by Destiny Diaz 4D
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.

Re: multiplying half reactions

Posted: Sat Mar 16, 2019 4:23 pm
by Rehan Chinoy 1K
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.

Re: multiplying half reactions

Posted: Sat Mar 16, 2019 4:24 pm
by dgerges 4H
you don't multiply cell potential, only the coefficients in the half reaction