In the reaction given below:
$3 {B r}_{2} + 6 C O_{3}^{2 -} + 3 H_{2} O ⟶ 5 {B r}^{⊖} + B r O_{3}^{⊖} + 6 H C O_{3}^{⊖}$

bromine is oxidised and carbonate is reduced

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bromine is reduced and water is oxidised

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bromine is neither reduced nor oxidised

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bromine is both reduced and oxidised

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Solution

The correct option is C bromine is both reduced and oxidised
The reaction is given below:
$3 {B r}_{2} + 6 C O_{3}^{2 -} + 3 H_{2} O ⟶ 5 {B r}^{⊖} + B r O_{3}^{⊖} + 6 H C O_{3}^{⊖}$
0 -1 +5
It is a disproportionation reaction and hence, $B r_{2}$ is reduced as well as oxidised.

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Similar questions

3 B r_{2} + 6 C O_{3}^{2 -} + 3 H_{2} O \to 5 B r^{-} + B r O_{3}^{-} + 6 H C O_{3}^{-}

3 B r_{2} + 6 C O_{3}^{2 -} + 3 H_{2} O \to 5 B r^{⊖} + B r O_{3}^{⊖} + 6 H C O_{3}^{⊖}

In the following reaction

3Br₂ + 6CO₃^2- + 3H₂O → 5Br ^-+ BrO₃^- + 6HCO₃^-

3 {B r}_{2} + 6 C O_{3}^{2 -} + 3 H_{2} O ⟶ 5 {B r}^{⊖} + B r O_{3}^{⊖} + 6 H C O_{3}^{⊖}

3 B r_{2} + 6 C O_{3}^{2 -} + 3 H_{2} O \to 5 B r^{-} + B r O_{3}^{-} + 6 H C O_{3}^{-}

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