  # 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?

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Updated on: September 25th, 2023 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. 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.

Table of content ## Electricity required for the oxidation of 1 mole of H2O to O2 and 1 mole of FeO to Fe2O3

The question states “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.

(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

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.

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.

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