Redox Reaction and Redox Reaction Examples
Redox Reaction and Redox Reaction Examples: Such a reaction in which oxidation and reduction reactions are taking place simultaneously is called a redox reaction. So in simple words, a redox reaction is an electron transfer process.
Those substances which are oxidized, reduce another substance, so they are called reductants, thus the substance which gets reduced is called oxidants.
Redox Reaction Examples
CuSO4 + Zn → ZnSO4+ Cu
(Here Zn and ZnSO4 are being oxidised and CuSO4 and Cu are being reduced.)
eg. Fe2O3 + 3CO → 2Fe + 3CO2
(Here Fe2O3 and 2Fe are being reduced and 3CO and 3CO2 are being oxidised.)
Zn+CuSO4 → ZnSO4 + Cu
In this reaction, Cu is formed by giving up Zn2 electrons, Zn2+ and Cu2+ gaining 2 electrons which are oxidation and reduction reactions respectively. Hence it is called a redox reaction.
Oxidation Number
The number of electrons lost or gained by an atom in the formation of a compound is called its oxidation number.
If electrons are being lost by an atom, the oxidation number is represented by a positive number and if electrons are being gained, the oxidation number is represented by a negative number.
Oxidation and Reduction
Reduction
The process of taking hydrogen or other positively charged element or radical by a substance or giving up oxygen or other negative electronegativity or radical is called reduction.
In reduction, the valency of any one element of the substance decreases.
Example:
reduction of chlorine
Cl2 + H2 ——> 2HCl
reduction of iodine
I2 + Hg ——-> HgI2
Oxidation
The process of taking oxygen or other negative electronegativity or radical by a substance or giving up a hydrogen or other positive element or radical is called oxidation.
In oxidation, the valency of any one element of the substance increases.
Example:
oxidation of carbon
C + O2 ——> CO2
oxidation of ferrous chloride
2FeCl2 + Cl2 ——-> 2FeCl3
Applications of Redox Reactions
Production of Chemicals: Many chemicals of our daily needs like caustic soda, chlorine, fluorine, etc. are produced by electrolysis which takes place by redox reactions.
In The Extraction of Metals: By using suitable reducing agents, metal oxides can be reduced to metals. For example- Fe2O3 is reduced to Fe by using coke as a reducing agent in the blast furnace.
