What mass of aluminum can be deposited by the passage of a constant current of 5.00 A through a Al(NO₃)₃ solution for 2.00 hours?

Question

Quizplus · Accepted Answer

The mass of aluminum deposited can be calculated using Faraday's laws of electrolysis. The charge passed is 5.00 A * 7200 s = 36000 C. The molar mass of Al is 26.98 g/mol, and it requires 3 moles of electrons (3 * 96485 C/mol) to deposit 1 mole of Al. The mass deposited is (36000 C / (3 * 96485 C/mol)) * 26.98 g/mol = 3.36 g.

What Mass of Aluminum Can Be Deposited by the Passage