First slide

Faraday's Laws

Question

Al₂O₃ is reduced by electrolysis at low potentials and high currents. If 4.0 × 10⁴ amperes of current is passed through molten Al₂O₃ for 6 hours. What mass of aluminium is produced ? (Assume 100% current efficiency. At mass of Al = 27g mol^–1)

Easy

Solution

Total Coulombs passed = 4 x 10⁴ x 6 x 60 x 60 = 864 x 10⁶
$mass of Al produced = \frac{9 \times 864 \times 10^{6}}{96500}$

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