6M.1

[JamieVu_2C]

A student was given a standard Cu(s)|Cu2+(aq) half-cell and another half-cell containing an unknown metal M in 1.00M M(NO3)2(aq) and formed the cell M(s)|M+(aq)||Cu2+(aq)|Cu(s). The cell potential was found to be -0.689 V. What is the value of E(M2+/M)?

In this problem, since Cu2+(aq)/Cu(s) is written on the right side of the cell diagram, it should be the cathode. So, Cu2+(aq)/Cu(s) should be written as a reduction half reaction. However, the textbook solutions says that it is the anode and is instead written as an oxidation half reaction. Why is this? If the Cu2+(aq)/Cu(s) electrode is on the right of the cell diagram, then shouldn't it be the cathode?

[Brian Tangsombatvisit 1C]

You're right, if the Cu half reaction is written on the right side of the equation, it should be the cathode. This is probably a typo in the textbook as the solutions manual writes it on the left side of the cell diagram, making it the anode.

[Jessica Esparza 2H]

Has anyone confirmed if this is a typo? I was confused when looking at the answer key.

[Alexis Webb 2B]

I am not sure if it is a typo, but I was wondering what answer would you get if the Cu2+/Cu is the cathode so that I can check mine.

[Daniel Honeychurch1C]

In 6 L.3 of the textbook, it says that a positive cell potential indicates that the right side of the cell diagram is the cathode. Conversely, a negative cell potential indicates that the left side of the cell diagram in the cathode. In this question, the cell potential is negative (-0.689 V), so the left side of the cell diagram (M 2+/M) is the cathode.