Aluminium oxide may be electrolysed at 1000^ to furnish aluminium metal (Atomic mass = 27 amu ; 1 Faraday = 96,500 Coulombs ). The cathode reaction is - Chemistry MCQ AIEEE 2026 | ExamTest.live

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Aluminium oxide may be electrolysed at 100 0^{\circ} C to furnish aluminium metal (Atomic mass = 27 amu; 1 Faraday = 96, 500 Coulombs). The cathode reaction is: Al^{3 +} + 3 e^{-} \to Al To prepare 5.12 kg of aluminium metal by this method would require:

Solution & Step-by-step Explanation

According to Faraday's First Law of Electrolysis: Q = n \times F = (\frac{mass}{Equivalent mass}) \times F Given:Mass m = 5.12 kg = 5120 g Atomic mass of Al = 27 g/mol n -factor for Al^{3 +} \to Al is 3 .Equivalent mass = 27/3 = 9 g/eq . Q = \frac{5120}{9} \times 96500 Q = 568.88 \times 96500 \approx 5.49 \times 1 0^{7} C

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Aluminium oxide may be electrolysed at 100 0^{\circ} C to furnish aluminium metal (Atomic mass = 27 amu; 1 Faraday = 96, 500 Coulombs). The cathode reaction is: Al^{3 +} + 3 e^{-} \to Al To prepare 5.12 kg of aluminium metal by this method would require:

5.49 \times 1 0^{7} C of electricity

1.83 \times 1 0^{7} C of electricity

5.49 \times 1 0^{4} C of electricity

5.49 \times 1 0^{1} C of electricity

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