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A2 Chemistry - Electrode potentials

Hello,

I've done some questions before on electrode potentials for A-Level Chemistry, and some of them have completely baffled me as I have no idea how to approach them. These questions are basically the ones that give you several half-equations and their standard electrode potentials, and you have to explain the reaction that occurs.

For example, see question 5 (d) on this paper, 2 (d) (iv) on this paper and 3 (b) (i) on this paper.

I have no idea how to apply the data in these questions! Could someone show me how to do it? :smile:
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denise3693
Fe2+ + 2e– → Fe Eo__= –0.44 V
Cu2+ + 2e– → Cu Eo__= +0.34 V

The more negative electrode will release elctrone to th emore positive one in an anticlockwise direction if the two equations are listed as above with the more negative on top.

Then you scale the equations to balance the electrons and move around anticlockwise.

So in the above equations:
The top equation gets reversed to
Fe → Fe2+ + 2e-and the second stays as it is
Cu2+ + 2e– → Cu

so the overall equation becomes
Fe + Cu2+ --> Fe2+ + Cu

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