The electrolysis of molten AlCl₃ for 3.25 hr with an electrical current of 15.0 A produces ________ g of aluminum metal.

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Quizplus · Accepted Answer

The mass of aluminum produced can be calculated using Faraday's law of electrolysis. The molar mass of aluminum (Al) is 26.98 g/mol, and it has a valency of 3, meaning 3 moles of electrons are required to produce 1 mole of aluminum. The total charge (Q) passed through the electrolyte is current (I) times time (t), Q = I × t = 15.0 A × 3.25 × 3600 s = 175500 C. Since 1 mole of electrons corresponds to 96500 C (Faraday constant), the moles of electrons used are 175500 C / 96500 C/mol = 1.818 moles. Since it takes 3 moles of electrons to produce 1 mole of Al, the moles of Al produced are 1.818 moles of electrons / 3 = 0.606 moles of Al. Finally, the mass of Al produced is 0.606 moles × 26.98 g/mol = 16.4 g.

The Electrolysis of Molten AlCl3 for 3

The Electrolysis of Molten AlCl₃ for 3