A current of 13.0 A is passed through molten magnesium chloride for 16.0 h.How many moles of magnesium metal could be produced via this electrolysis?

Question

Quizplus · Accepted Answer

First, we need to calculate the amount of charge (Q) passed through the electrolyte using the equation Q = It, where I = current and t = time.

Q = 13.0 A x 16.0 h x 3600 s/h = 748800 C

Since the electrolysis of magnesium chloride produces magnesium metal at the cathode, we can use Faraday's laws of electrolysis to determine the amount of magnesium metal produced:

moles of magnesium metal = Q / (2 x F x E)

where F is the Faraday constant (96485 C/mol e-) and E is the electrode efficiency, which is assumed to be 100% in this case.

moles of magnesium metal = 748800 C / (2 x 96485 C/mol e-) = 3.883 mol

Therefore, the answer is B) 3.88 mol.

A Current of 13