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  1. moles Al = 54000 g / 27 g/mol= 2000

    Al3+ + 3e- >> Al

    for every 3 faradays consumed 1 mole of Al is liberated

    2000 x 3 = 6000 faradays

    6000 x 96500 /C/F) = 193000000 coulombs

    193000000/ 500 = 386000 s

Time required to produce 54 kg of Al(s) in an electrolytic cell?

How long would it take to produce 54 kg of Al metal by the reduction of Al3+ in an electrolytic cell using a current of 500 amps?
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