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At the top of page 575 in the textbook, for the reaction Cu(s)|Cu2+(aq)||Zn2+(aq)|Zn(s), it says that Cu(s) is the cathode and Zn (s) is the anode. But shouldn't it be the other way around since Cu is being oxidized and Zn is being reduced?
The reason why the cathode and anode are switched is because for this example they are writing the reverse cell potential and demonstrating how that would be setup. In general however, it should be anode||cathode, so you are correct.
But on the same page it says "A negative cell potential indicates that the right-hand electrode in the cell diagram is the anode (the site of oxidation, where electrons leave the cell)", but isn't the right-hand electrode being reduced in the example?
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