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<!--td {border: 1px solid #ccc;}br {mso-data-placement:same-cell;}--> An example of a disproportionation reaction is:

JEE MAIN 2019
  1. 2KMnO4K2MnO4+MnO2+O2
  2. 2NaBr+Cl22NaCl+Br2
  3. 2CuBrCuBr2+Cu
  4. 2MnO4+10I+16H+2Mn2++5I2+8H2O

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Solution

The correct option is C 2CuBrCuBr2+Cu
(A) 2KMnO4K2MnO4+MnO2+O2

-In this reaction, manganese has +7 oxidation state in KMnO4 and +6 and +4 oxidation states in K2MnO4 and MnO2 respectively. This indicates manganese is only getting reduced. And O is getting oxidised from 2 to 0. So, this reaction is not a disproportionation reaction.

(B) 2MnO4+10I+16H+2Mn2++5I2+8H2O
-In this reaction, manganese has +7 oxidation state in MnO4 and +2 oxidation state in the product side.
And I is getting oxidised from 1 to 0.
So, this reaction is not a disproportionation reaction.

(C) 2CuBrCuBr2+Cu
-In this reaction, copper is +1 in CuBr and +2 oxidation state in CuBr2and zero oxidation state elemental form. This implies, In this reaction copper is getting both oxidized as well as reduced. Therefore, this reaction is an example of a disproportionation reaction.

(D) 2NaBr+Cl22NaCl+Br2
In this reaction, Br is getting oxidised from 1 to 0 and Cl is getting reduced from 0 to 1. Hence, this is not a disproportionation reaction.

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