An example of a disproportionation reaction is :

  • Option 1)

    2CuBr\rightarrow Cubr_{2}+Cu

  • Option 2)

    2KMnO_{4}\rightarrow K_{2}MnO_{4}+MnO_{2}+O_{2}

  • Option 3)

    2MnO^{-}_{4}+10I^{-}+16H^{+}\rightarrow 2Mn^{2+}+5I_{2}+8H_{2}O

  • Option 4)

    2NaBr+CI_{2}\rightarrow 2NaCI+Br_{2}

Answers (2)

 

Disproportionation Reactions -

A special type of redox reaction in which one oxidation state is simultaneously oxidised and reduced. One of the reacting substances in a disproportionation reaction always contains an element that can exist in at least three oxidation states. 

- wherein

2H_{2}\ O_{2}(aq)\rightarrow 2H_{2}\ O(l)+O_{2}(g)

+1     -1                     +1    -2               0

 

 

 

Disproportionation reactions are those where oxidation & reduction both occur simultaneously

                             2CuBr\rightarrow CuBr_{2}+Cu

oxidation state :       +1                 +2               0

of Cu

 

\therefore option (1) is correct


Option 1)

2CuBr\rightarrow Cubr_{2}+Cu

Option 2)

2KMnO_{4}\rightarrow K_{2}MnO_{4}+MnO_{2}+O_{2}

Option 3)

2MnO^{-}_{4}+10I^{-}+16H^{+}\rightarrow 2Mn^{2+}+5I_{2}+8H_{2}O

Option 4)

2NaBr+CI_{2}\rightarrow 2NaCI+Br_{2}

option 1

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