Amount of electricity used during the following reaction?

Question

A steady current was passed through molten CoSO4 until 2.27 g of metallic cobalt was produced. Calculate the number of coulombs of electricity used.

Answer 1

Each Co needs 2 electrons to change from Co++ to Co atom.
1 mol Co atoms are formed by using 2 mol electrons or 2 Faradays or 2 x 96500 Coulombs.

1 mol Co is 58.9 g.
So 2.27 g are formed by using (2 x 96500 x 2.27 / 58.9) Coulombs.

Answer 2

96,500 Coulombs will give you half a mole of Co metal (because it's a 2+ ion).

Now work out how many moles 2.27g is.