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?

3618 seconds

Explanation:

According to mole concept:

1 mole of an atom contains number of particles.

We know that:

Charge on 1 electron =

Charge on 1 mole of electrons =

At cathode:

1 mole of aluminium is deposited by =

Thus 0.15 moles of aluminium is deposited by =

To calculate the time required, we use the equation:

where,

I = current passed =12.0 A

q = total charge =

t = time required in seconds = ?

Putting values in above equation, we get:

Hence, the amount of time required to produce 4.00 g of aluminum metal from the electrolysis of molten with an electrical current of 12.0 A is 3618 seconds

a chemical reaction

explanation: