(7.15a) What mass of copper is plated out in the electrolysis of CuSO4, in the same time that it takes to deposit 1.00g of Ag in a silver coulometer that is arranged in series with CUSO4 cell? (7.15b) If a current of 1.00 A is used, how many minutes is required to plate out this quantity of copper? Molar Mass (g/mol): Cu 63.546 Ag 107.87 Analysis/Strategy: ampere & time mol e (or Faraday) ® mol coulombs ® Cu mass of Cu time to plate out Cu = time to plate out 1.00 g Ag (in series with CUSO4 cell) Reduction half-reaction of silver metal: Ag"(aq) + e ® Ag(s) Reduction half-reaction of copper metal: Cu"“(aq) 1+2, + Cu(s)

(7.15a) What mass of copper is plated out in the electrolysis of CuSO4, in the same time that it takes to deposit 1.00g of Ag in a silver coulometer that is arranged in series with CUSO4 cell? (7.15b) If a current of 1.00 A is used, how many minutes is required to plate out this quantity of copper? Molar Mass (g/mol): Cu 63.546 Ag 107.87 Analysis/Strategy: ampere & time mol e (or Faraday) ® mol coulombs ® Cu mass of Cu time to plate out Cu = time to plate out 1.00 g Ag (in series with CUSO4 cell) Reduction half-reaction of silver metal: Ag"(aq) + e ® Ag(s) Reduction half-reaction of copper metal: Cu"“(aq) 1+2, + Cu(s)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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