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Are we allowed to change the sign (as in multiply by -1) of the standard cell potentials of the half reactions if we are looking for the standard cell potential of the reverse half reaction? I had thought that this was not possible because reversing a reduction half reaction makes it an oxidation reaction since the e- would be on the products side.
Technically, you can flip a reaction and change the by multiplying it by negative 1, as you said. Thus, by using the equation of , you can see that the standard cell potentials for reactions and their reverse counterparts are equal and opposite.
Yes you can flip the reaction and the sign of Eo, but if in the case you are determining cell potentials and you happen to be using the equation Ecell = Ecathode - Eanode, you would just keep the signs of the E cathode and E anode as given because the negative sign in the equation accounts for the sign flip.
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