(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
(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
Chemistry by OpenStax (2015-05-04)
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ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 22E: The mass of three different metal electrodes, each from a different galvanic cell, were determined...
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Question
![(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
coulombs ® mol e¯ (or Faraday) ® mol
®
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*2(aq) +
e
® Cu(s)
Answer: Mass of copper plated out =
g (3 sig fig)
Minutes required to plate out
copper using 1.00 ampere =
minutes (3 sig fig)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F28b0c32b-120e-4886-93a2-e1b26d860aab%2F98cd1b3e-d42e-4dba-ae57-6a8765191d32%2Ftgnd59_processed.jpeg&w=3840&q=75)
Transcribed Image Text:(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
coulombs ® mol e¯ (or Faraday) ® mol
®
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*2(aq) +
e
® Cu(s)
Answer: Mass of copper plated out =
g (3 sig fig)
Minutes required to plate out
copper using 1.00 ampere =
minutes (3 sig fig)
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