9 Redox Reaction Example: Detailed Explanations

In this article, we are going to see, what redox reaction example is with their explanation in detail.

• Reaction of Iron and copper sulphate
• Formation of Hydrogen fluoride
• Reaction of Zinc and copper sulphate
• Reaction of Iron and Hydrogen Peroxide
• Reaction of Copper sulphate and potassium iodide
• Reaction of Hydrogen sulphide and chlorine
• Reaction of Arsenous acid and Bromate
• Reaction of Potassium permanganate and Ferrous sulphate
• Reaction of Manganese ion and Chlorine trioxide
• Reaction of Hydrogen peroxide and Perchloric acid

The word redox itself shows that there are two processes involved in the reaction. Those are Oxidation and Reduction and are going on at the same time during the course of the reaction.

Oxidation: During the reaction, some of the atoms change their oxidation number or loss of electrons takes place or there is the addition of an electronegative element or there is a gain of oxygen or loss of hydrogen, then it is called as oxidation.

Reduction: During the reaction, the gain of electrons takes place by some of the atoms or addition of electropositive element or gain of hydrogen or loss of oxygen.

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Redox Reaction Example

Reaction of Iron and copper sulphate

In the reaction of iron and copper sulphate, the oxidation number changes from 0 to +2. Shows increases in the oxidation number of ferrous. The decrease in oxidation number is shown by copper from +2 to 0. It is a redox reaction because the Oxidation number shows an increase and decrease of the reactants.

Formation of Hydrogen fluoride

In the above reaction, the oxidation reaction is shown by hydrogen as its oxidation number changes from 0 to +1 on the other hand reduction reaction is shown by fluorine as its oxidation number changes from +1 to 0. It is a redox reaction because the Oxidation number shows an increase and decrease of the reactants.

Reaction of  Zinc and copper sulphate

During the reaction of Zinc and copper sulphate, the oxidation reaction is shown by zinc as its oxidation number changes from 0 to +2 on the other hand reduction reaction is shown by copper as its oxidation number changes from +2 to 0. The oxidation number of reactant species increases and others decreases therefore it’s a redox reaction.

Reaction of  Iron and Hydrogen Peroxide

In the above reaction, the oxidation number increases from +2 to +3, or loss of electrons takes place, hence its oxidation, shown by iron. The oxidation number decreases from 0 to +1 or gain of electrons taking place, is reduction shown by hydrogen peroxide.  

Reaction of  Copper sulphate and potassium iodide

In the reaction of Copper sulphate and potassium iodide, oxidation and reduction take place at the same time it is a redox reaction. Oxidation half-reaction is shown by iodide while reduction half-reaction is shown by copper.

Reaction of  Hydrogen sulphide and chlorine

During the reaction of Hydrogen sulphide and chlorine, the loss of hydrogen is called oxidation, is shown by H2S and gain of hydrogen is called reduction is shown by chlorine. As the reduction and oxidation reactions take place at the same time it is considered as a redox reaction.

Reaction of  Arsenous acid and Bromate

In the above reaction the oxidation no, of As changes by +3 to +5 and the oxidation number of Br changed from +5 to -1. It is a redox reaction as the Oxidation number of one reactant species increases while the other decreases.

Reaction of  Potassium permanganate and Ferrous sulphate

In the reaction of Potassium permanganate and Ferrous sulphate, the oxidation number changes from +2 to +3. Shows increases in the oxidation number of ferrous. The decrease in oxidation number is shown by manganese from +7 to +2.

Reaction of  Manganese ion and Chlorine trioxide

This reaction required an acidic medium. Oxidation number changes from +2 to +4 of one reactant species while others decrease from +5 to +4. It is a redox reaction because the Oxidation number shows an increase and decrease of the reactants.

Reaction of  Hydrogen peroxide and Perchloric acid

In the above reaction oxidation number changes from -1 to 0. It shows an increase by 1. The oxidation number of chlorine trioxide is decreasing from +7 to +3 It is a redox reaction because the Oxidation number shows an increase and decrease of the reactants. This reaction required an acidic medium.

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Frequently Asked Questions:

Question: What are oxidizing agents?

Answer: The oxidizing agents are,

A substance or a reagent that causes oxidation of another substance or species and itself undergoes reduction are termed an oxidizing agent or oxidant. It is an electron acceptor species.

Question: What are reducing agents?

Answer: The reducing agents are,

A substance or a reagent which cause the reduction of another substance or species and itself undergoes oxidation are termed a reducing agent or reductant. It is an electron donor species.

Question: What are the examples of oxidizing and reducing agents?

Answer: The examples of oxidizing and reducing agents are as follows,

Oxidizing agents:  O₂, O₃, H₂SO₄, HNO₃, KMnO₄, H₂O₂ etc.

Reducing agents: LiH, LiAlH_4, NaH, CaH₂ etc.

Question: What are the types of redox reactions?

Answer: The four types of redox reactions :

Combination reactions

Disproportion reactions

Decomposition reactions

Displacement reactions.

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