Aluminum metal can be produced by the electrolytic reduction of Al ions in an acidic…
CHEMISTRY · Multi-part · AP · Chemistry · Thermodynamics and Electrochemistry · Thermodynamics and Electrochemistry
Problem
Aluminum metal can be produced by the electrolytic reduction of Al3+ ions in an acidic aqueous solution according to the half-reaction:
Al3+(aq) + 3 e− → Al(s)
A technician wishes to obtain exactly 1.08 g of aluminum (the molar mass of Al is 26.98 g mol−1) using a constant current of 10.0 A.
(a) Calculate the number of moles of electrons required to produce 1.08 g of aluminum.
(b) Determine the total electrical charge, in coulombs, that must pass through the cell to supply the electrons calculated in part (a).
(c) Calculate the time, in minutes, for which the 10.0 A current must be maintained to obtain the desired mass of aluminum.