How many kilograms of aluminum metal can be produced by the electrolysis of Al₂O₃ using a current of 100 amperes for 24 hours?

Question

Quizplus · Accepted Answer

The mass of aluminum produced can be calculated using Faraday's laws of electrolysis. The molar mass of aluminum (Al) is approximately 27 g/mol, and it has a valency of 3, meaning 3 moles of electrons are required to produce 1 mole of aluminum. The amount of charge (Q) passed is given by Q = It, where I is the current (100 A) and t is the time in seconds (24 hours = 24 × 3600 s). The charge of one mole of electrons (the Faraday constant) is approximately 96485 C/mol. Using these values, the mass of aluminum produced can be calculated as follows:$$ \text{Mass} = \left( \frac{It}{nF} \right) \times \text{Molar mass of Al} $$$$ \text{Mass} = \left( \frac{100 \times 24 \times 3600}{3 \times 96485} \right) \times 27 $$This calculation yields a mass of approximately 0.81 kg, making option A the correct answer.

How Many Kilograms of Aluminum Metal Can Be Produced by the Electrolysis