## 6th edition, 14.55

$E_{cell} = E_{cell}^{\circ}-\frac{RT}{nF}\ln Q$

Hai-Lin Yeh 1J
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### 6th edition, 14.55

A 1.0 m NiSO4(aq) solution was electrolyzed by using inert electrodes. Write (a) the cathode reaction; (b) the anode reaction. (c) With no overpotential or passivity at the electrodes, what is the minimum potential that must be supplied to the cell for the onset of electrolysis?

I'm not sure how the solutions manual got the cathode and anode reaction just from being given NiSO4. For example, where did the SO4 go and why did we use the reaction for 2H2O? Also, can someone explain the "strategy" in the solutions manual more clearly?

Griffin Carter 2I
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Joined: Wed Nov 14, 2018 12:23 am

### Re: 6th edition, 14.55

So we can assume that Ni is going to be formed at the cathode because that is the only substance that would form a solid via electrolysis in this reaction. However, the book uses the oxidation of water at the anode because it has a more negative standard E potential than the SO4- standard potential. This more negative value should be used because it has lower energy requirements to oxidize.

Hai-Lin Yeh 1J
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Joined: Fri Sep 28, 2018 12:16 am
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### Re: 6th edition, 14.55

What do you mean by it has lower energy requirements to oxidize?

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