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(C) $1$. Analyze the oxidation states of the elements in the reaction: $MnO_4^- + H^+ + Br^- \longrightarrow Mn^{2+}(aq.) + Br_2 \uparrow$.$2$. In $Mn

Vedclass · Accepted Answer

$C$: Either intermolecular redox reaction or displacement reaction.

Vedclass · Answer

(C) $1$. Analyze the oxidation states of the elements in the reaction: $MnO_4^- + H^+ + Br^- \longrightarrow Mn^{2+}(aq.) + Br_2 \uparrow$.$2$. In $MnO_4^-$,the oxidation state of $Mn$ is $+7$. In $Mn^{2+}$,it is $+2$. Thus,$Mn$ is reduced.$3$. In $Br^-$,the oxidation state of $Br$ is $-1$. In $Br_2$,it is $0$. Thus,$Br$ is oxidized.$4$. Since two different elements ($Mn$ and $Br$) are undergoing oxidation and reduction in separate species,this is an intermolecular redox reaction.$5$. According to the definitions provided,the correct assignment is $C$.

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