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(C) In the reaction: $H_2O + \overset{0}{Br_2} 	o HO\overset{+1}{Br} + H\overset{-1}{Br}$$1$. The oxidation state of $Br$ in $Br_2$ is $0$.$2$. In $H

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It is both oxidized and reduced.

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(C) In the reaction: $H_2O + \overset{0}{Br_2} 	o HO\overset{+1}{Br} + H\overset{-1}{Br}$$1$. The oxidation state of $Br$ in $Br_2$ is $0$.$2$. In $HOBr$,the oxidation state of $Br$ is $+1$ (Oxidation).$3$. In $HBr$,the oxidation state of $Br$ is $-1$ (Reduction).Since $Br_2$ undergoes both oxidation and reduction,it is a disproportionation reaction.

Which of the following best describes the behavior of bromine in the reaction given below?
$H_2O + Br_2 \to HOBr + HBr$

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Which of the following best describes the behavior of bromine in the reaction given below?$H_2O + Br_2 \to HOBr + HBr$

Similar Questions

Auto-oxidation of bleaching powder gives:

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

In the reaction $3I_2 + 6NaOH \to NaIO_3 + 5NaI + 3H_2O$,which substance acts as the oxidizing agent?

Which of the following best describes the behavior of bromine in the reaction given below?$H_2O + Br_2 \to HOBr + HBr$

What is a disproportionation reaction? Give an example.

Vedclass Test Series

Exam Paper Generator

Online Exam Module

Which of the following best describes the behavior of bromine in the reaction given below?
$H_2O + Br_2 \to HOBr + HBr$

Which of the following best describes the behavior of bromine in the reaction given below?
$H_2O + Br_2 \to HOBr + HBr$