Applied Chemistry E4050 Principles of Industrial Electrochemistry Problem Set # 1 Aluminum metal is produced by electrolysis of alumina dissolved in a mixture of molten fluorides at 970 oC. The free enthalpy (Gibbs function) change for the reaction: Al2O3 (soln) + 3/2C(c) = 2Al(l) + 3/2CO2 (g) under these conditions is: ?G = 698.7 kJ/mol. The observed cell voltage is 4.5 volts and the cathodic current efficiency is 90%. Calculate: a) the reversible cell voltage (Erev); b) the theoretical energy consumption per kg of aluminum; c) the current required for the production of 1 metric ton of aluminum per day; d) the electrical energy actually required per metric ton of aluminum; e) the voltages efficiency and the energy efficiency of the process. f) the amount of heat dissipated in the process assuming that the enthalpy required for the reaction above is ?rH = 1,263.77 kJ mol-1.
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