2016 Midterm #8A

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Michelle_Nguyen_3F
Posts: 40
Joined: Wed Sep 21, 2016 2:59 pm

2016 Midterm #8A

Postby Michelle_Nguyen_3F » Sun Feb 12, 2017 5:18 pm

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

Postby Chem_Mod » Sun Feb 12, 2017 5:22 pm

Yes, you would need to identify the half reactions, but the 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

Madeline_Foo_3J
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Joined: Wed Sep 21, 2016 3:00 pm

Re: 2016 Midterm #8A

Postby Madeline_Foo_3J » Mon Feb 13, 2017 3:02 pm

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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Re: 2016 Midterm #8A

Postby Abigail_Low_1A » Mon Feb 13, 2017 9:14 pm

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)


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