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If you are just using the cathode - anode equation you don't need to flip any numbers because the minus sign takes care of that. But, if you are using the method of writing out the half reactions and making the net equation, you'll have to make sure you flip the E for the oxidation half reaction.
If using the equation E(cell) = E(cathode) - E(anode) and using reduction values found in the appendix or on the sheet he will give us on the test, then I'm pretty sure that there is no need to flip the anode cell potential value when accounting for oxidation. In this case you would not need to change the sign from Ecell given for standard reduction.
What I found was confusing was that in Youtube videos, the teachers would be adding the cell potentials while the book has us subtract the anode from the cathode. These are both the same thing it is just that, like others have said, you don't change the standard potential sign when you are using the subtraction method.
Cindy Adiwidjaja 1B wrote:I know that E is given, however, why do we need to flip the sign when we are trying to use the E for oxidation?
Honestly, for me, I feel like it's easier to do Cathode-anode, that way you don't have to worry about changing the E value given.
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