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Redox Reactions - Practice Questions & MCQ

Edited By admin | Updated on Sep 25, 2023 25:23 PM | #NEET

Quick Facts

  • Types of Redox Reactions is considered one of the most asked concept.

  • 25 Questions around this concept.

Solve by difficulty

Which of the following is a redox reaction?

Which one of the following reactions does not come under hydrolysis type reaction ?

 

Concepts Covered - 1

Types of Redox Reactions

The different types of redox reactions are:

  • Decomposition Reaction
  • Combination Reaction
  • Displacement Reaction
  • Disproportionation Reactions

Decomposition Reaction
This is the reaction which involves the breakdown of a compound into different compounds. Some examples of this type of reaction are:

2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \stackrel{\Delta}{\longrightarrow} 2 \mathrm{H}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})
2 \mathrm{KClO}_{3}(\mathrm{s}) \stackrel{\Delta}{\longrightarrow} 2 \mathrm{KCl}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{g})

This must be noted here that all decomposition reactions are not redox reactions. For example, decomposition of calcium carbonate is not a redox reaction.
\mathrm{CaCO}_{3}(\mathrm{s}) \stackrel{\Delta}{\longrightarrow} \mathrm{CaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{g})

Combination Reaction
These types of reactions are the opposite of decomposition reaction and hence involve the combination of two compounds to form a single compound. Some examples include:

\mathrm{C}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{g}) \stackrel{\Delta}{\longrightarrow} \mathrm{CO}_{2}(\mathrm{g})
\mathrm{CH}_{4}(\mathrm{g})+2 \mathrm{O}_{2}(\mathrm{g}) \stackrel{\Delta}{\longrightarrow} \mathrm{CO}_{2}(\mathrm{g})

Displacement Reaction
Displacement reactions, also known as replacement reactions, involve compounds and the replacing of elements. They occur as single and double replacement reactions. In other words, in theses type of reactions, an atom or an ion in a compound is substituted by another element. The general representation of this reaction is as follows:

\mathrm{X}+\mathrm{YZ} \rightarrow \mathrm{XZ}+\mathrm{Y}

Disproportionation Reactions

Disproportionation reactions are those reactions in which a single element in one oxidation state is simultaneously oxidized and reduced. Some examples include:

\mathrm{P}_{4}(\mathrm{s})+3 \mathrm{OH^{-}}(\mathrm{aq})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{PH}_{3}(\mathrm{g})+3 \mathrm{H}_{2} \mathrm{PO}_{2}^{-}
\begin{array}{r}{\mathrm{S}_{8}(\mathrm{s})+12 \mathrm{OH}(\mathrm{aq}) \rightarrow 4 \mathrm{S}^{2-}(\mathrm{aq})+2 \mathrm{S}_{2} \mathrm{O}_{3}^{2}(\mathrm{aq})} \: {+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})}\end{array}

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Types of Redox Reactions

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Types of Redox Reactions

Chemistry Part II Textbook for Class XI

Page No. : 270

Line : 8

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