Chem help please.3?

Question

Calculate the mass of Li formed by electrolysis of molten LiCl by a current of 7.6 * 10 ^ 4 * A flowing for a period of 30 h. Assume the electrolytic cell is 90 % efficient.

i did this and calculated the mass of Li to be 5.3x10^5 g Li

part 2:

what is the minimum voltage required to drive the reaction?

I need help with part 2 please

Answer 1

For part 2, you are dealing with finding the the voltage for each half reaction.

Since you are making LiCl, you know that you are dealing with an oxidation and reduction (I got these standard reduction potentials from google)

Oxidation would occur for Lithium: Li(s) ---> Li_{(aq) + e}^- E^°= +1.36 V

Reduction would occur for the Chlorine: Cl₂ + 2e^- ---> 2Cl^- E^°= -3.04 V

E_cell=E_red - E_ox -3.04 V - (+1.36 V)= -4.40 V to make it favorable, it should be positive, so +4.40V