# How much electricity is required in coulomb for the oxidation of? (i) 1 mole of H2O to O2? (ii) 1 mole of FeO to Fe2O3?

By Ritesh|Updated : November 13th, 2022

The electricity required in coulomb for the oxidation of 1 mole of H2O to O2 is 1.93 x 105 C and 1 mole of FeO to Fe2O3 is 9.65 x 104 C.

(i) H2O → 2H+ + ½ O2 + 2e-

1 mol 2F

Electricity required to oxidise 1 mole H2O to O2 = 2F

= 2 x 96500 C

= 193000 C

In simplification we get:

= 1.93 x 105 C

(ii) 2FeO + ½ O2 → Fe2O3

2Fe2+ → 2Fe3+ + 2e-

2 mol 2F

Electricity required to oxidise 2 moles FeO to Fe2O3 = 2F

Electricity required to oxidise 2 moles FeO to Fe2O3 = 1F = 96500 C

= 9.65 x 104 C

### Types of Redox Reactions

Redox reactions are oxidation-reduction chemical processes in which the oxidation states of the reactants change. Redox is a shortened version of reduction oxidation. Two distinct processes—a reduction process and an oxidation process - can be used to describe all redox reactions.

Redox or Oxidation-Reduction processes always involve simultaneous oxidation and reduction reactions. In a chemical reaction, the material that is being reduced is referred to as the reducing agent, while the substance that is being oxidized is the oxidising agent.

The different types of redox reactions are:

1. Decomposition Reaction
2. Combination Reaction
3. Displacement Reaction
4. Disproportionation Reactions

Summary:

## How much electricity is required in coulomb for the oxidation of? (i) 1 mole of H2O to O2? (ii) 1 mole of FeO to Fe2O3?

The electricity required in coulomb for the oxidation of 1 mole of H2O to O2 is 1.93 x 105 C and 1 mole of FeO to Fe2O3 is 9.65 x 104 C. Oxidation is a process that involves the addition of oxygen or any electronegative element or the removal of hydrogen or any electropositive element.