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Choose the balanced reaction for disproportionation of \mathrm{Br_{2}} in alkaline medium:

Option: 1

3 \mathrm{Br}_2+6 \mathrm{OH}^{-} \rightarrow 5 \mathrm{Br}^{-}+\mathrm{BrO}^{3-}+3 \mathrm{H}_2 \mathrm{O}


Option: 2

\mathrm{Br}_2+\mathrm{OH}^{-} \rightarrow \mathrm{Br}^{-}+\mathrm{BrO}^{3-}+\mathrm{H}_2 \mathrm{O}


Option: 3

\mathrm{Br}_2+5 \mathrm{OH}^{-} \rightarrow 4 \mathrm{Br}^{-}+\mathrm{BrO}^{3-}+2 \mathrm{H}_2 \mathrm{O}


Option: 4

2 \mathrm{Br}_2+4 \mathrm{OH}^{-} \rightarrow 5 \mathrm{Br}^{-}+\mathrm{BrO}^{3-}+\mathrm{H}_2 \mathrm{O}


Answers (1)

best_answer

The unbalanced reaction for the disproportionation of \mathrm{Br_{2}} is : \mathrm{Br}_2 \rightarrow \mathrm{Br}^{-}+\mathrm{BrO}^{3-}

Balancing the charge and atoms: 3 \mathrm{Br}_2+6 \mathrm{OH}^{-} \rightarrow 5 \mathrm{Br}^{-}+\mathrm{BrO}^{3-}

Adding water to balance H atoms: 3 \mathrm{Br}_2+6 \mathrm{OH}^{-} \rightarrow 5 \mathrm{Br}^{-}+\mathrm{BrO}^{3-}+3 \mathrm{H}_2 \mathrm{O}

Posted by

sudhir kumar

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