A current was passed for 5 hours through two electrolytic cells connected in series. The first cell contains AuCl3 and second cell CuSO4 solution. If 9.85 g of gold was deposited in the first cell, what amount of copper gets deposited in the second cell? Also calculate magnitude of current in ampere.Given: Atomic mass of Au = 197 amu and Cu = 63.5 amu.
A current was passed for 5 hours through two electrolytic cells connected in series. The first cell contains AuCl3 and second cell CuSO4 solution. If 9.85 g of gold was deposited in the first cell, what amount of copper gets deposited in the second cell? Also calculate magnitude of current in ampere.Given: Atomic mass of Au = 197 amu and Cu = 63.5 amu.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 77AP
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A current was passed for 5 hours through two electrolytic cells connected in series. The first cell contains AuCl3 and second cell CuSO4 solution. If 9.85 g of gold was deposited in the first cell, what amount of copper gets deposited in the second cell? Also calculate magnitude of current in ampere.
Given:
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