20. Electrochemistry
Electroplating
10PRACTICE PROBLEM
(a) Assuming that the electrolytic cell has 78% efficiency, what is the mass of Cs formed from the electrolysis of molten CsCl using a current of 2.5×103 A for a period of 12 h? (b) Determine the minimum voltage needed to drive the reaction.
Cs+ + e– → Cs E°red = –3.03 V
Cl2 + 2 e– → 2 Cl– E°red = –1.36 V
(a) Assuming that the electrolytic cell has 78% efficiency, what is the mass of Cs formed from the electrolysis of molten CsCl using a current of 2.5×103 A for a period of 12 h? (b) Determine the minimum voltage needed to drive the reaction.
Cs+ + e– → Cs E°red = –3.03 V
Cl2 + 2 e– → 2 Cl– E°red = –1.36 V