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Types of Redox Reactions - (Concept)

The different types of redox reactions are:

Decomposition Reaction
Combination Reaction
Displacement Reaction
Disproportionation Reactions

Decomposition Reaction
This is the reaction that 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 species to form a single compound. Some examples include:

$\mathrm{C}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{g}) \stackrel{\Delta}{\longrightarrow} \mathrm{CO}_{2}(\mathrm{g})$
$3Mg(s)+N_2(g)\rightarrow Mg_3N_2(s)$

Displacement Reaction
Displacement reactions, also known as replacement reactions, involve compounds and the replacement 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.

Some examples include:

$\\\mathrm{Zn(s)+ CuSO_4(aq)\rightarrow ZnSO_4(aq)+Cu(s)(Metal\ displacement)} \\\mathrm{Na(s)+ H_2O(l)\rightarrow NaOH(aq)+H_2(g)(Non-Metal\ displacement)}$

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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Exam	Chapter
JEE MAIN	Redox Reaction and Electrochemistry

A.	$\mathrm{NaCl + KNO _{3} \rightarrow NaNO _{3}+ KCl}$
B.	$\mathrm{CaC _{2} O _{4}+2 HCl \rightarrow CaCl _{2}+ H _{2} C _{2} O _{4}}$
C.	$\mathrm{Mg ( OH )_{2}+2 NH _{4} Cl \rightarrow MgCl _{2}+2 NH _{4} OH}$
D.	$\mathrm{Z n+2 A g C N \rightarrow 2 A g+Z n(C N)_{2}}$

A.	XeF₆ + H₂O → XeOF₄ + 2HF
B.	XeF₆ + 2H₂O → XeO₂F₂ + 4HF
C.	XeF₄ + O₂F₂ → XeF₆ + O₂
D.	XeF₂ + PF₅ → [XeF]⁺ PF₆⁻

A.	Na
B.	H
C.	NaH
D.	Not a redox reaction.

A.	Cl
B.	F
C.	Neither
D.	The reaction is not redox

A.	$Be\rightarrow Be^{2+}+2e^{-}$
B.	$K^{+}+e^{-}\rightarrow K$
C.	$3H_2+N_2\rightarrow 2NH_3$
D.	$2Mg+O_2\rightarrow 2MgO$

A.	Oxidation half reaction
B.	Reduction half reaction
C.	both
D.	none

A.	$2Cl^{-}\rightarrow Cl_2+2e^{}-$
B.	$N_2+3H_2\rightarrow 2NH_3$
C.	$F_2+2e^{-}\rightarrow 2F^{-}$
D.	$Na\rightarrow Na^{+}+e^{-}$

A.	$2Mg+O_2\rightarrow 2MgO$
B.	$H_2O \rightarrow H_2+\frac{1}{2}O_2$
C.	$3F_2+3H_2O\rightarrow O_3+6HF$
D.	$2KClO_3\rightarrow 2KCl+3O_2$

A.	$Fe+CuSO_4\rightarrow Cu+FeSO_4$ - Metal displacement
B.	$3Cl_{2\left ( g \right )}+6OH^-\rightarrow 5Cl^-+ClO_3^-+3H_2O$ - Disproportionation
C.	$2AgCl_{\left ( s \right )}\overset{sunlight}{\rightarrow}2Ag+Cl_{2(g)}$ - Decomposition
D.	$C+O_2\rightarrow CO_2$ - Non-metal displacement

A.	Formation of ozone from atmospheric oxygen in presence of sunlight
B.	Redox of $H_{2}SO_{4}$ with $NaOH$
C.	Combination of dinitrogen with dioxygen of 2000K.
D.	Reaction of $[Co(H_{2}O)_{6} ]Cl_{3}$ with $AgNO_{3}$

A.	$2 \mathrm{H}_{2} \mathrm{O}_{2} \rightarrow 2 \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}$
B.	$2 \mathrm{NO}_{2}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{HNO}_{3}+\mathrm{HNO}_{2}$
C.	$\mathrm{MnO}_{4}^{-}+4 \mathrm{H}^{+}+3 \mathrm{e}^{-} \rightarrow \mathrm{MnO}_{2}+2 \mathrm{H}_{2} \mathrm{O}$
D.	$3 \mathrm{MnO}_{4}^{2-}+4 \mathrm{H}^{+} \rightarrow 2 \mathrm{MnO}_{4}^{-}+\mathrm{MnO}_{2}+2 \mathrm{H}_{2} \mathrm{O}$

A.	in a circular path
B.	in a wavy path
C.	in a straight line path
D.	with an accelerated velocity.

A.	$2Fe\left ( OH \right )_{3}\overset{\Delta }{\rightarrow}Fe_2O_3+3H_2O$
B.	$Pb(NO_3)_2+Fe\rightarrow Fe(NO_3)_2+Pb$
C.	$2KI+Br_2\rightarrow 2KBr+I_2$
D.	$3Mg+N_2\rightarrow Mg_3N_2$

A.	1-r,2-q,3-p,4-s
B.	1-q,2-s,3-p,4-r
C.	1-q,2-p,3-s,4-r
D.	1-s,2-q,3-p,4-r

A.	Sr
B.	Cl
C.	S
D.	None

A.	$Cu^{2+}/Fe,Fe^{2+}/Cu$
B.	$Cu/Fe,Cu^{2+}/Fe^{2+}$
C.	$Fe^{2+}/Fe,Cu^{2+}/Cu$
D.	$Fe/Cu,Fe^{2+}/Cu^{2+}$

A.	b,d
B.	a,b,d
C.	a,d
D.	a,b

A.	$\mathrm{Cu_{2}I_{2}}$
B.	$\mathrm{Cu_{2} I_{3}}$
C.	$\mathrm{C u I}$
D.	$\mathrm{C u\left(I_{3}\right)_{2}}$

A.	Disproportionation Reaction
B.	Decomposition Reaction
C.	Metal Displacement Reaction
D.	Non-Metal Displacement Reaction

A.	$\mathrm{H}^{+}+\mathrm{Cl}^{-} \rightarrow \mathrm{HCl} \\$
B.	$2 \mathrm{Ca}+\mathrm{O}_2 \rightarrow 2 \mathrm{CaO} \\$
C.	$\mathrm{Ni}+4 \mathrm{CO} \rightarrow \mathrm{Ni}(\mathrm{CO})_4 \\$
D.	$\mathrm{CuSO}_4+\mathrm{Kl} \rightarrow 2 \mathrm{Cul}+\mathrm{I}_2+\mathrm{K}_2 \mathrm{SO}_4$

A.	Both the statements are true and Statement II is not the correct reason for Statement I.
B.	Both the statements are true and Statement II is the correct reason for Statement I.
C.	Both the statements are false.
D.	Statement II is true and statement I is false.

A.	$\mathrm{Cl}_2+\mathrm{SnCl}_2 \rightarrow \mathrm{SnCl}_4 \\$
B.	$\mathrm{Cu}+2 \mathrm{AgNO}_3 \rightarrow \mathrm{Cu}\left(\mathrm{NO}_3\right)_2+2 \mathrm{Ag} \\$
C.	$2 \mathrm{KClO}_3 \rightarrow 2 \mathrm{KCl}+\mathrm{O}_2 \\$
D.	$\mathrm{AgCl}+2 \mathrm{NH}_3 \rightarrow\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)_2\right] \mathrm{Cl}$

A.	I is correct II is false
B.	I is false II is true
C.	Both I & II are true
D.	Neither I nor II are true

A.	I is the Correct explanation of II
B.	II is the Correct explanation of I
C.	I false II is True
D.	I is True but Il is false

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Types of Redox Reactions - (Concept)

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