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(C) In the given reaction: $2NaBr + MnO_2 + 2H_2SO_4 \longrightarrow MnSO_4 + Na_2SO_4 + Br_2 + 2H_2O$$1$. The oxidation state of $Mn$ changes from $+

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for either intermolecular redox reaction or displacement reaction.

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(C) In the given reaction: $2NaBr + MnO_2 + 2H_2SO_4 \longrightarrow MnSO_4 + Na_2SO_4 + Br_2 + 2H_2O$$1$. The oxidation state of $Mn$ changes from $+4$ in $MnO_2$ to $+2$ in $MnSO_4$ (reduction).$2$. The oxidation state of $Br$ changes from $-1$ in $NaBr$ to $0$ in $Br_2$ (oxidation).$3$. Since two different elements are undergoing oxidation and reduction in the same reaction,it is an intermolecular redox reaction.$4$. It can also be classified as a displacement reaction where $Mn$ displaces $Br$ or vice versa in terms of electron transfer context.Therefore,the correct classification is $C$.

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$2NaBr + MnO_2 + 2H_2SO_4 \longrightarrow MnSO_4 + Na_2SO_4 + Br_2 + 2H_2O$

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Assign $A$,$B$,$C$,$D$ from the given type of reaction.$2NaBr + MnO_2 + 2H_2SO_4 \longrightarrow MnSO_4 + Na_2SO_4 + Br_2 + 2H_2O$