## 2016 Midterm #8A

Michelle_Nguyen_3F
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Joined: Wed Sep 21, 2016 2:59 pm

### 2016 Midterm #8A

A standard electrochemical cell is made by placing a silver electrode into a 1.0 M Ag + solution and a cadmium electrode into a 1.0 M Cd2+ solution. What is the redox reaction and what is the maximum potential produced by this cell? Be sure to show half reactions?

How do we tell which is being oxidized/reduced just based on the information above? Or, are we supposed to figure out what is being oxidized/reduced based on the Enot values, which I assume will be given to us?

Chem_Mod
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### Re: 2016 Midterm #8A

Yes, you would need to identify the half reactions, but the $E^{\circ}$ values of the corresponding reactions will be given. Then you would decide based on those values which one would be an anode and which one would be a cathode

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### Re: 2016 Midterm #8A

Why did they add the two values together in this problem? I thought Enot was solved by E(cathode)-E(anode) ?

Abigail_Low_1A
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Joined: Sat Sep 24, 2016 3:01 am

### Re: 2016 Midterm #8A

You only do E(cathode)-E(anode) if the values given are standard reduction potentials. If the half reactions given are reduction reactions (with electrons on the reactant side), then the E values given with it are reduction potentials. However, the E value given for the anode is for the oxidation reaction, so it's the not the reduction potential. In this case, E_cell is just the sum of E(cathode)+E(anode)