The diagram shows a cell used to extract aluminium from its ore, bauxite, which contains aluminium oxide. A steady current of 15.0 A was allowed to pass through the molten aluminium oxide for 2 hours. At the cathode: Al³⁺ + 3e⁻ → Al. [1 Faraday = 96 500 C; Ar of Al = 27]

1. aWrite the chemical formula of aluminium oxide. [1]
2. bThe anode has to be replaced because it is used up in the process. Write an equation for the reaction that causes the anode to be used up. Include state symbols. [2]
3. cCalculate the charge, in coulombs, that was passed through the molten aluminium oxide. [2]
4. dCalculate the number of Faradays used. [2]
5. eCalculate the mass of aluminium that will be produced. [2]

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