Redox and Equivalent ConceptHard

Question

In the disproportionation reaction (unbalanced), $Br_{2} + OH^{-} \rightarrow Br^{-} + BrO_{3}^{-} + H_{2}O$

The ratio of Br2 molecules undergoing oxidation and reduction is

Options

A.5:1
B.1:5
C.2:3
D.3:2

Solution

Oxidation:$Br_{2} + 12OH^{-} \rightarrow 2BrO_{3}^{-} + 6H_{2}O + 10e^{-}$

Reduction:$Br_{2} + 2e^{-} \rightarrow 2Br^{-}1 \times 5$

Net reaction: $6Br_{2} + 12OH^{-} \rightarrow 2BrO_{3}^{-} + 10Br^{-} + 6H_{2}O$

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