Aluminium oxide may be electrolysed at `1000^(@)`C to furnish aluminium metal (Atomic mass = 27 amu, 1 Faraday = 96500 Coulomb). The cathode reaction is `Al^(3+) + 3e^(-) rightarrow Al`. To prepare 5.12 kg of aluminium metal by this method would require:

Options

A. `5.49xx10^(4)C` of electricity
B. `5.49xx10^(1)C` of electricity
C. `5.49xx10^(7)C` of electricity
D. `1.83xx10^(7)C` of electricity.

Answer

C

Explanation

`Al^(3+)+3e^(-)rarrAl`
`3xx96500 27g`
To produce 27g of Al, electricity required
`=3xx96500C`
`therefore` To produce 5.12kg of Al, electricity required
`=(3xx96500)/(27)xx5.12xx10^(3)C`
`=5489.78xx10^(3)C=5.49xx10^(7) C`