In the reaction 3Br_2 + 6CO_3^{2-} + 3H_2O to | vedclass

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(D) Assigning oxidation numbers to the species in the reaction:$3\overset{0}{Br}_2 + 6CO_3^{2-} + 3H_2O 	o 5\overset{-1}{Br}^- + \overset{+5}{Br}O_3^

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Bromine is both reduced and oxidized.

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(D) Assigning oxidation numbers to the species in the reaction:$3\overset{0}{Br}_2 + 6CO_3^{2-} + 3H_2O 	o 5\overset{-1}{Br}^- + \overset{+5}{Br}O_3^- + 6HCO_3^-$$1$. The oxidation state of $Br$ changes from $0$ in $Br_2$ to $-1$ in $Br^-$,which is a decrease in oxidation number,representing reduction.$2$. The oxidation state of $Br$ changes from $0$ in $Br_2$ to $+5$ in $BrO_3^-$,which is an increase in oxidation number,representing oxidation.Since $Br_2$ undergoes both oxidation and reduction,it is a disproportionation reaction.

In the reaction $3Br_2 + 6CO_3^{2-} + 3H_2O \to 5Br^- + BrO_3^- + 6HCO_3^-$,which of the following is true?

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