Electrolytic cells use electricity to cause a nonspontaneous redox reaction to o

Question

Electrolytic cells use electricity to cause a nonspontaneous redox reaction to occur. An electrolytic cell is constructed using the following components: a power source, such as a battery, the substance that will undergo electrolysis, and two inert electrodes (usually platinum), which serve as the electrical connection between the power source and the substance undergoing electrolysis. When electricity is applied to a molten binary salt during electrolysis, the cation will be reduced and the anion will be oxidized. If more than one cation is present, only the one with highest reduction potential will be reduced. Similarly, if more than one anion is present, only the one with the highest oxidation potential will be oxidized.

What substance is produced at the anode during the electrolysis of molten calcium bromide, CaBr2? Assume standard conditions.

Express your answer as a chemical formula.

Explanation / Answer

If we have the electrolylis of CaBr2 this means that we are actually working with the ions Ca2+ and Br-. So all we have to do, is see which one has the lowest standard reduction potential, this will be the substance that's is being oxidized, and the substance that is in the anode:

E°Ca = -2.76 V
E°Br = +1.09 V

This means that Ca is being oxidized by Br and the reaction taking place is the following:

Ca --------> Ca2+ + 2e-
Br2 + 2e- --------> 2Br-

The Calcium is in the anode.

Hope this helps

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