Aluminium oxide may be electrolysed at $1000 \, ^\circ C$ to furnish aluminium metal (At. Mass $= 27 \, amu$; $1 \, F = 96,500 \, C$). The cathode reaction is $Al^{3+} + 3e^- \to Al^0$. To prepare $5.12 \, kg$ of aluminium metal by this method would require:
- A$5.49 \times 10^7 \, C$ of electricity
- B$1.83 \times 10^7 \, C$ of electricity
- C$5.49 \times 10^4 \, C$ of electricity
- D$5.49 \times 10^1 \, C$ of electricity
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