How many seconds are required to produce 5.00 g of aluminum metal from the electrolysis of molten AlCl₃ with an electrical current of 15.0 A?

Question

Quizplus · Accepted Answer

To find the time, use the formula: time = (moles of electrons × Faraday's constant) / current. First, calculate moles of Al: 5.00 g / 26.98 g/mol = 0.185 mol. Al requires 3 moles of electrons per mole of Al, so 0.185 mol Al × 3 = 0.555 mol electrons. Using Faraday's constant (96485 C/mol), total charge = 0.555 mol × 96485 C/mol = 53553.675 C. Time = 53553.675 C / 15.0 A = 3570.245 s, which is approximately 3.57 × 10³ s.

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