Which of the following reactions is a disprop | vedclass

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(B) disproportionation reaction is a type of redox reaction in which the same element in a single oxidation state is simultaneously oxidized and reduc

Vedclass · Accepted Answer

$Cl_2 + 2 OH^{-} \rightarrow ClO^{-} + Cl^{-} + H_2O$

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(B) disproportionation reaction is a type of redox reaction in which the same element in a single oxidation state is simultaneously oxidized and reduced.In the reaction $Cl_2 + 2 OH^{-} \rightarrow ClO^{-} + Cl^{-} + H_2O$:- The oxidation state of $Cl$ in $Cl_2$ is $0$.- In $ClO^{-}$,the oxidation state of $Cl$ is $+1$ (oxidation).- In $Cl^{-}$,the oxidation state of $Cl$ is $-1$ (reduction).Since the same element $(Cl)$ is both oxidized and reduced,this is a disproportionation reaction.

Which of the following reactions is a disproportionation reaction?

Similar Questions

Which of the following species can function both as an oxidizing as well as a reducing agent?

Refer to the periodic table and answer the following questions:
$(a)$ Select the possible non-metals that can show disproportionation reaction.
$(b)$ Select three metals that can show disproportionation reaction.

The species given below that does $NOT$ show disproportionation reaction is :

In the following reaction $P_4 + 3NaOH + 3H_2O \to PH_3 + 3NaH_2PO_2$,what happens to phosphorus?

Which of the following is not a disproportionation reaction?

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