How many faradays of electricity will be required to electrolyse completely 1 mol of molten `Al_(2)O_(3)` to produce Al metal and `O_(2)` gas ?

Explanation

Dissociation of `Al_(2)O_(3):underset("1 mol")(Al_(2)O_(3))hArrunderset("2 mol")(2Al^(3+))+underset("3 mol")(3O^(2-))`
`"1 gram - equivalent of "Al^(3+)" ions "-=(1)/(3)xx"1 mol "Al^(3+)" ions"`
So, 2 mol of `Al^(3+)` ions `-="6 g-eq of "Al^(3+)" ions."`
For the discharge 6g - eq of `Al^(3+)` ions, 6 F of electricity is required.
Hence, 6F of electricity will completely1 mol of `Al_(2)O_(3)`.