Question

What amount of electricity must be supplied to an electrolytic cell in order to produce 0.100Kg of Iron from Iron(III)oxide?

Answer 1

Answer:

4 v answer to the question ..I hope it's help you

Answer 2

Answer:

The amount of electricity must be supplied to an electrolytic cell in order to produce $0.100kg$  of Iron from Iron oxide is $1.195$.

Explanation:

The metal which coats on the other metal during the process of electrolysis comes from the electrolyte. The anode should be of the metal that has to be electroplated and the cathode should be of the metal on which the electroplating has to be done.

We know that $F=96500 \,C\, mol^{-1}$

RAM of Fe is $55.85$

Therefore, by Faraday law of thermodynamics, the amount of electricity must be supplied to an electrolytic cell in order to produce $0.100kg$  of Iron from Iron oxide is $1.195$.

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