Chemistry 10th Edition

Published by Brooks/Cole Publishing Co.
ISBN 10: 1133610668
ISBN 13: 978-1-13361-066-3

Chapter 21 - Electrochemistry - Exercises - Electrolytic Cells: General Concepts - Page 844: 26

Answer

8.39 g Ag

Work Step by Step

Charge $Q=I\times t= 2.78\,A\times 45.0\times60\,s$ $=7506\,C$ According to the equation $Ag^{+}+e^{-}\rightarrow Ag$ Charge of 1 mol electrons or 96500 C is required to produce 1 mol Ag or 107.87 g Ag. $\implies$ mass of silver that could be plated= $\frac{7506\,C}{96500\,C}\times 107.87\,g=8.39\,g$
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