Consider the following reaction,3Br_2 + 6CO_3 | vedclass

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(D) In the given reaction,the oxidation state of bromine $(Br_2)$ in the reactant side is $0$.When it changes to $BrO_3^-$,the oxidation state of brom

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Bromine is both reduced and oxidized

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(D) In the given reaction,the oxidation state of bromine $(Br_2)$ in the reactant side is $0$.When it changes to $BrO_3^-$,the oxidation state of bromine increases to $+5$,which indicates oxidation (loss of electrons).When it changes to $Br^-$,the oxidation state of bromine decreases to $-1$,which indicates reduction (gain of electrons).Since bromine undergoes both oxidation and reduction,this is a disproportionation reaction.Therefore,bromine is both reduced and oxidized.

Consider the following reaction,
$3Br_2 + 6CO_3^{2-} + 3H_2O \longrightarrow 5Br^{-} + BrO_3^- + 6HCO_3^-$
Which of the following statements is true regarding this reaction?

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Consider the following reaction,$3Br_2 + 6CO_3^{2-} + 3H_2O \longrightarrow 5Br^{-} + BrO_3^- + 6HCO_3^-$Which of the following statements is true regarding this reaction?