A galvanic cell is assembled from a zinc electrode in 1.0 M ZnSO (aq) and a copper…
CHEMISTRY · Multi-part · AP · Chemistry · Thermodynamics and Electrochemistry · Thermodynamics and Electrochemistry
Problem
A galvanic cell is assembled from a zinc electrode in 1.0 M ZnSO4(aq) and a copper electrode in 1.0 M CuSO4(aq), connected by a salt bridge. The cell delivers a constant current of 0.50 A for 40.0 min.
Atomic masses: Zn = 65.38 g mol−1; Cu = 63.55 g mol−1.
(a) Calculate the total charge that passes through the external circuit during the 40.0 min interval.
(b) Determine the number of moles of electrons transferred.
(c) Calculate the mass of zinc metal lost from the zinc electrode during this time.
(d) Calculate the mass of copper metal deposited on the copper electrode.
(e) If the zinc electrode initially had a mass of 5.00 g, determine the percentage of its original mass that remains after the 40.0 min discharge.