It will take 103 minutes to plate out 16. 22 g of al metal from a solution of al 3 using a current of 12. 9 amps in an electrolytic cell
Electrolytic cell, any device in which electrical energy is converted to chemical energy, or vice versa. Such a cell typically consists of two metallic or electronic conductors (electrodes) held apart from each other and in contact with an electrolyte (q.v.), usually a dissolved or fused ionic compound
First, look at the reaction to decided how many moles of electrons it will take:
Al3+ + 3e ------> Al(s)
It takes 3 electrons to convert 1 mole of Al3+
Next, figure out how many moles of Al metal you want:
I mole of Al mass = 26 g
1 g of Al will have = 1/26 moles
16. 22 g of al metal will have = 16.22 / 26 moles 0.624 moles
since , their are 3 electrons
0.624 x 3= 1.87 moles of electrons
using Faraday constant to find the number of coulombs (C) needed:
1 faraday = 96500 C per mole
1.87 x 96500 = 180455
Since, 1 amp = 1 C/sec,, time needed to supply a current of 12.9 amp will be
80455C / 12.9 C = 6236.82 sec = 103 minutes
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