Question

Reduction of 1 mole of \[\ce{MnO^-_4}\] to Mn²⁺ requires ______ coulombs of charge.

Answer 1

Reduction of 1 mole of \[\ce{MnO^-_4}\] to Mn²⁺ requires 482500 coulombs of charge.

Explanation:

The reduction of 1 mole of \[\ce{MnO^-_4}\] (permanganate ion) to Mn²⁺ requires 5 moles of electrons, and hence the charge required is

Q = 5F

= 5 × 96500

= 482500 C