Question

How many minutes will it take 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?

Answer 1

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

To learn more about electrolytic cell here

brainly.com/question/862677

#SPJ4