An industrial process electrolyzes molten in a fused-salt cell
CHEMISTRY · Multi-part · AP · Chemistry · Thermodynamics and Electrochemistry · Thermodynamics and Electrochemistry
Problem
An industrial process electrolyzes molten CrCl3 in a fused-salt cell. A current of 2.00 A is maintained for exactly 2.00 h.
Molar mass of Cr: 52.00 g mol−1
Faraday constant: F=9.6485×104Cmol−1
The only cathode reaction is Cr3++3e−→Cr(l).
(1) Part 1: a) Calculate the total charge delivered to the cell over the 2.00 h run.
(2) Part 2: b) Determine the number of moles of chromium metal produced.
(3) Part 3: c) Compute the mass of chromium collected at the cathode.
(4) Part 4: d) Suppose the current efficiency for chromium deposition is later found to be 88.0 %. Re-evaluate the actual mass of Cr obtained under this efficiency.