Redox Table

[smurphy1D]

If all of the reactions in the table represent reductions, for the oxidizing half reaction, it would be made negative, then would the sign in the Ecat-Eanode change to addition or would we subtract it?

[TimVintsDis4L]

If you are asking whether or not to change the sign when subtracting the anode from cathode then remember this simple rule.

When you are doing E(cell) = E(cathode) - E(anode), then you use the numbers given as is, and DO NOT change the sign based on whether its Oxidized or not.

For example

If your reactions are

Reduction : = -.40V
Oxidation : = -2.93V

Although the appendix gives the oxidation in the form of a reduction, you do not need to flip the sign like you might think. Instead leave it and subtratc

E= -.40V - (-2.93V)

Were you to flip the sign, then you would want to add the numbers

E= -.40V + (+2.93V)

Ultimately, you would get the same answer.

[Gabriella Bates 2L]

You can think about it both ways. If you keep the sign of Eanode as it is, then Ecell = Ecathode - Eanode. However, if you flip the sign of Eanode since it is an oxidation, then Ecell = Ecathode + Eanode. Just be clear which method you use and you will be fine!

[Sjeffrey_1C]

The equation takes into consideration that the values are reduction potential values, even though half of the reaction is actually in oxidation. Thus, you don't need to convert the values to oxidation potential.

[Martina]

If you already flip the value for the oxidation part of the reaction, then you just have to add them, or you can subtract the cathode from the anode for both reduction values. Either way it is the same, but it can get confusing.

[Eugene Chung 3F]

If all of the reactions in the table represent reductions, for the oxidizing half reaction, it would be made negative, then would the sign in the Ecat-Eanode change to addition or would we subtract it?

If you don't want to worry about changing the sign, it's easier to just do Ecat-Eanode and always consider the red. rxn for both anode and cathode.

[Althea Zhao 1B]

The equation for E(cell) allows you to use the given reduction potentials for each half-reaction: making E(anode) a negative value accounts for the oxidation sign change.