The cell reaction in a particular electrolysis is: Ag*(aq) + e-→ Ag°(s) After passing a certain amount of electricity through the cell, the mass of silver depos- ited is 0.13 28 g. How many mol(s) of silver metal has been deposited? a. How many silver atoms have been deposited? (The Avogadro number is 6.02×1023). с. How many electrons have been used in the electrolysis? If the electronic charge is 1.60 x 10-19 Coulomb, what is the total electrical charge used? If a constant current of 90 mA is used, how long has the electrolysis taken place? е.
The cell reaction in a particular electrolysis is: Ag*(aq) + e-→ Ag°(s) After passing a certain amount of electricity through the cell, the mass of silver depos- ited is 0.13 28 g. How many mol(s) of silver metal has been deposited? a. How many silver atoms have been deposited? (The Avogadro number is 6.02×1023). с. How many electrons have been used in the electrolysis? If the electronic charge is 1.60 x 10-19 Coulomb, what is the total electrical charge used? If a constant current of 90 mA is used, how long has the electrolysis taken place? е.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.78QE
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