Calculate the mass in grams of aluminum produced by passing 375 amperes of current through a molten mixture containing Al³⁺ ions for 300 seconds. (1 F = 96500 C/mol e^-)

Question

Quizplus · Accepted Answer

First, we need to calculate the number of electrons that pass through the circuit:

375 A x 300 s = 112500 C

Using the Faraday constant, we can convert this to the number of moles of electrons:

112500 C / 96500 C/mol = 1.167 mol e-

Since the Al ions gain 3 electrons to form neutral Al atoms, the number of moles of Al produced is one-third of the number of moles of electrons:

1.167 mol e- / 3 = 0.389 mol Al

The molar mass of Al is 26.98 g/mol, so the mass of Al produced is:

0.389 mol x 26.98 g/mol = 10.5 g

Therefore, the answer is D.

Calculate the Mass in Grams of Aluminum Produced by Passing