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For the electrolysis of CuCl2 (molten) to form Cu(s) and Cl2(g): E°Cu2+/Cu = 0.339 V E°Cl-/Cl2 = 1.360 V What minimum voltage must be used to carry out the reaction? If 1.5V is used, how much electrical energy (in kJ) will be used to produce 2g of  Cl2(s)?

For the electrolysis of CuCl2 (molten) to form Cu(s) and Cl2(g): E°Cu2+/Cu = 0.339 V E°Cl-/Cl2 = 1.360 V What minimum voltage must be used to carry out the reaction? If 1.5V is used, how much electrical energy (in kJ) will be used to produce 2g of  Cl2(s)?

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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For the electrolysis of CuCl2 (molten) to form Cu(s) and Cl2(g):
E°Cu2+/Cu = 0.339 V
E°Cl-/Cl2 = 1.360 V

What minimum voltage must be used to carry out the reaction? If 1.5V is used, how much electrical energy (in kJ) will be used to produce 2g of  Cl2(s)?

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