Al2O3 is reduced by electrolysis at low potentials and high currents. If 4.0 $ \times $ 104 amperes of current is passed through molten Al2O3 for 6 hours, what mass of aluminium is product? (Assume 100% current efficiency, at mass of Al = 27 g mol$-$1).

Question

Al₂O₃ is reduced by electrolysis at low potentials and high currents. If 4.0 $ \times $ 10⁴ amperes of current is passed through molten Al₂O₃ for 6 hours, what mass of aluminium is product? (Assume 100% current efficiency, at mass of Al = 27 g mol^$-$1).

8.1 $ \times $ 10⁴ g

2.4 $ \times $ 10⁵ g

1.3 $ \times $ 10⁴ g

9.0 $ \times $ 10³ g

Solution

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