A laboratory technician operates an electrolytic cell containing CuSO (aq) at 25 °C
CHEMISTRY · Multi-part · AP · Chemistry · Thermodynamics and Electrochemistry · Thermodynamics and Electrochemistry
Problem
A laboratory technician operates an electrolytic cell containing CuSO4(aq) at 25 °C. A steady current of 1.50 A is passed through the cell for 45.0 min.
Molar mass of Cu: 63.55 g mol−1
Faraday constant: F=9.6485×104 C mol−1
(a) Calculate the total electric charge that passes through the cell during the 45.0 min interval. Report your answer in coulombs.
(b) Determine the number of moles of electrons that flow through the external circuit in that time.
(c) The half-reaction occurring at the cathode is Cu2+ + 2 e− → Cu(s). Calculate the mass of copper metal deposited on the cathode after 45.0 min.