DEPARTMENT OF CHEMICAL ENGINEERING COURSE: Electrochemical Engr. COURSE NO.: CHEG 295-01; CHEG 320-02 INSTRUCTOR: Prof. J. M. Fenton Faraday’s Law The basis for electrochemical theory and technology are Faraday’s laws of electrolysis which formed a crucial link between chemistry and electricity. These laws are called in honor of Michael Faraday (1791-1867) who formulated them during 1833 and 1834: 1. The amount of chemical change produced by electrolysis is proportional to the total amount of charge passed through the cell. 2. The amount of chemical change produced is proportional to the equivalent weight of the substance undergoing chemical change. W= W I t z F ItA zF = weight in grams of the compound undergoing electrolysis = current in amperes; A = atomic weight = elapsed time of electrolysis in seconds = number of charges involved in the elementary reaction = Faraday’s constant, 96,493.5 coulombs/equivalent For engineering purposes, the value of the Faraday will be rounded off to 96,500 coulombs/equivalent. Example Problem #1: Calculate the daily aluminum production of a 150,000 ampere aluminum cell which operates at a current efficiency of 89%. The cell reaction is 2Al 2 0 3 + 3 C = 4 Al + 3 CO 2 Answer: ItA W = εc zF (1.5 x 10 A )(24 x 60 x 60 sec)(26.985 = 0.89 (3 )(96,500 ) day 5 geq gmol A sec geq gm gmole ) = 1.08 x 10 6 gm ton or 1.18 day day Example Problem #2 The electrolysis of water at high pressure is used to produce hydrogen and oxygen of very high purity. For a cell voltage of 1.78V, what is the power consumption in kwhrs per cubic meter of hydrogen gas at standard conditions of temperature and pressure? Answer: )( ( lit ) / 22.414 gmol 1m 3 of H 2 @ STP = (1m 3 )(100 cm 10 3 m 3 Faradays Law → (44.615 )(96,500 )(2 ) = 8.61 x 10 gmol m3 Since Power Current X Voltage: coul geq geq gmol (8.61 x 10 (3600 ) = 44.615 gmol 6 coul m3 )(1.78V )(1 )(10 ) 6 coul m3 sec hr cm 3 lit 3 watt kW waH⋅sec coul⋅volt ) = 4.26 kw − hr m 3 @STP