In the reaction,MnO_{4(aq)}^{-} + Br_{(aq)}^{ | vedclass

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(D) The given reaction is $MnO_{4(aq)}^{-} + Br_{(aq)}^{-} \rightarrow MnO_{2(s)} + BrO_{3(aq)}^{-}$.In $MnO_{4}^{-}$,the oxidation state of $Mn$ is $

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$Br^{-1}$ to $Br^{+5}$

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(D) The given reaction is $MnO_{4(aq)}^{-} + Br_{(aq)}^{-} \rightarrow MnO_{2(s)} + BrO_{3(aq)}^{-}$.In $MnO_{4}^{-}$,the oxidation state of $Mn$ is $x + 4(-2) = -1$,so $x = +7$.In $MnO_{2}$,the oxidation state of $Mn$ is $x + 2(-2) = 0$,so $x = +4$.In $Br^{-}$,the oxidation state of $Br$ is $-1$.In $BrO_{3}^{-}$,the oxidation state of $Br$ is $x + 3(-2) = -1$,so $x = +5$.Therefore,the oxidation number of bromine changes from $Br^{-1}$ to $Br^{+5}$.

In the reaction,$MnO_{4(aq)}^{-} + Br_{(aq)}^{-} \rightarrow MnO_{2(s)} + BrO_{3(aq)}^{-}$,the correct change in oxidation number of the species involved is

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