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In the reaction
$3 \mathrm{Br}_{2}+6 \mathrm{CO}_{3}^{2-}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow 5 \mathrm{Br}^{-}+\mathrm{BrO}_{3}^{-}+6 \mathrm{HCO}_{3}^{-}$
Options:
$3 \mathrm{Br}_{2}+6 \mathrm{CO}_{3}^{2-}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow 5 \mathrm{Br}^{-}+\mathrm{BrO}_{3}^{-}+6 \mathrm{HCO}_{3}^{-}$
Solution:
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Verified Answer
The correct answer is:
Bromine is both reduced and oxidised.
$\begin{aligned}
3 \mathrm{Br}_{2}+6 \mathrm{CO}_{3}^{2-}+3 \mathrm{H}_{2} \mathrm{O} & \rightarrow \\
5 \mathrm{Br}^{-} &+\mathrm{BrO}_{3}^{-}+6 \mathrm{HCO}_{3}^{-}
\end{aligned}$
O.N. of $\mathrm{Br}_{2}$ changes from 0 to -1 and +5 , hence it is reduced as well as oxidised.
3 \mathrm{Br}_{2}+6 \mathrm{CO}_{3}^{2-}+3 \mathrm{H}_{2} \mathrm{O} & \rightarrow \\
5 \mathrm{Br}^{-} &+\mathrm{BrO}_{3}^{-}+6 \mathrm{HCO}_{3}^{-}
\end{aligned}$
O.N. of $\mathrm{Br}_{2}$ changes from 0 to -1 and +5 , hence it is reduced as well as oxidised.
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