## Problem 14.21c

Daniel_Sands3L
Posts: 13
Joined: Fri Sep 25, 2015 3:00 am

### Problem 14.21c

In problem 14.21c, the problem provides the following cell diagram for us to find the cell potential: $Hg_{(l)}|Hg_{2}Cl_{2}_{(s)}|Cl^{-}_{(aq)}||Hg^{2+}_{(aq)}|Hg_{(l)}$.

How would you perform the oxidation at the anode provided that $Hg_{2}Cl_{2}_{(s)}$ is oxidized to $Cl^{-}_{(aq)}$? I'm a bit stuck here.

Chem_Mod
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### Re: Problem 14.21c

Cl isn't the ion undergoing redox in this diagram. On the left, you have Hg-> Hg+ and on the right, you have Hg-> Hg 2+. In this case, Hg is being both oxidized and reduced.

Daniel_Sands3L
Posts: 13
Joined: Fri Sep 25, 2015 3:00 am

### Re: Problem 14.21c

Is the Cl- ion in the cell diagram shown as the product of the oxidation half reaction then? Why is it included?

Ronald Yang 2F
Posts: 86
Joined: Fri Sep 25, 2015 3:00 am

### Re: Problem 14.21c

Because the Cl- is necessary for the oxidation half-reaction to occur. You also include species that is needed in the half-reaction. Also, on the right side resembling the cathode, isn't it Hg22+ -> Hg?