How many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten alcl3 with an electrical current of 12.0 a? how many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten alcl3 with an electrical current of 12.0 a? 3.57 × 103 1.19 × 103 9.00 2.90 × 105 27.0

A=

Step-by-step explanation:

Write the electrolysis reaction for Al

Find moles of Al using the molecular weight of Aluminum (26.981 g/mol)

Calculate moles of charge using the relation of the electrolysis reaction.

Using Faraday's Constant to calculate the quantity of electricity (Coulombs)

Finally, you can obtain the seconds using electrical current of 12 A (12 C/s)

I’m pretty sure the answer is counter steer.