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Electrochemical Cell Potential Under Non-Standard Conditions

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Consider the electrochemical cell:
Pt|Cr2+(0.2752 M), Cr3+(1.705 M)||Co2+(0.2008 M)|Co
a. What is the cell potential (hint: you can solve the problem by half-reactions or by the over-all reaction, both will give you the same answer so you can double check yourself)?
b. Is the cell galvanic or electrolytic (must show math in part (a) to get credit for answer)?

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Solution Summary

This solution contains step-by-step instructions on how to obtain reduction and oxidation half-reactions from the cell notation, how to obtain the cell potential under standard conditions using tabulated tables, and how to correct the cell potential for non-standard conditions using the Nernst equation. Detailed calculations are contained in the attached Word file.

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Please see attached World file as there are equations involved in the calculations that does not show up here.

A. I will do this the over-all reaction way as I feel it is easier:

From the cell notation the anode is Always written on the left side of the double line and the cathode is on the right side.

So Anode is Cr2+/Cr3+ couple. This is where oxidation occurs. Write an oxidation half-reaction where the electrons are on the product side (because oxidation means loss of ...

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