The electrolysis of molten AlCl₃for 3.25 hr with an electrical current of 15.0 A produces
G of aluminum metal.

Question

The electrolysis of molten AlCl₃for 3.25 hr with an electrical current of 15.0 A produces G of aluminum metal.

Quizplus · Accepted Answer

The amount of aluminum produced can be calculated using Faraday's law of electrolysis:

moles of Al = (current x time)/(96500 x charge of Al ion)

First, we need to find the charge on the Al ion:

AlCl3 → Al3+ + 3 Cl-

The charge on the Al ion is 3+.

Next, we can plug in the values:

moles of Al = (15.0 A x 3.25 hr)/(96500 C/mol x 3+) 
moles of Al = 0.00455 mol

Finally, we can convert moles to grams using the molar mass of Al:

mass of Al = 0.00455 mol x 26.98 g/mol 
mass of Al = 0.122 g

Converting to grams to grams:

0.122 g x 1000 = 122 g

Therefore, the answer is A) 16.4 (rounded to the nearest tenth).

The Electrolysis of Molten AlCl3 for 3