Question

When 0.1 mol \[\ce{MnO^{2-}_4}\] is oxidised, the quantity of electricity required to completely oxidise \[\ce{MnO^{2-}_4}\] to \[\ce{MnO^-_4}\] is ______.

Options

• 96500 C

• 2 × 96500 C

• 9650 C

• 96.50 C

Answer 1

When 0.1 mol \[\ce{MnO^{2-}_4}\] is oxidised, the quantity of electricity required to completely oxidise \[\ce{MnO{^{2-}_{4}}}\] to \[\ce{MnO^-_4}\] is 9650 C.

Explanation:

The oxidation of \[\ce{MnO^{2-}_4}\] to \[\ce{MnO^{2-}_4}\] involves a 1-electron change per molecule.

\[\ce{MnO^{2-}_4 -> MnO^4− + e-}\]

So, for 0.1 mol of \[\ce{MnO^{2-}_4}\], the charge required is:

Q = n × F

= 0.1 × 96500

= 9650 C