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For question 14.41 part (a), why is the Cu2+ with lower concentration the anode and Cu2+ with higher concentration the cathode? I thought you would want it the other way around since it would flow from high concentration to low concentration and you would want that to be anode to cathode.
You want e- to flow anode to cathode. At the anode Cu(s) > Cu2+ + 2e-. At the cathode Cu2+ + 2e- > Cu(s). So the anode  is a product and cathode  is a reactant. Since you want postive E and Q=P/R, so, using the eq, you can see that anode should always have lower .
The flow of electrons is not the same as the "flow" of the Cu2+. The electrons will flow towards the side with higher concentration of Cu2+ so that the copper ions there can get reduced to form Cu(s) and therefore reducing the concentration of Cu2+ in that cell.
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