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(C) In the given reaction: $MnO_2 + 2NaCl + 2H_2SO_4 \longrightarrow MnSO_4 + Na_2SO_4 + 2H_2O + Cl_2 \uparrow$$1$. Oxidation state of $Mn$ changes fr

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for either intermolecular redox reaction or displacement reaction.

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(C) In the given reaction: $MnO_2 + 2NaCl + 2H_2SO_4 \longrightarrow MnSO_4 + Na_2SO_4 + 2H_2O + Cl_2 \uparrow$$1$. Oxidation state of $Mn$ changes from $+4$ in $MnO_2$ to $+2$ in $MnSO_4$ (Reduction).$2$. Oxidation state of $Cl$ changes from $-1$ in $NaCl$ to $0$ in $Cl_2$ (Oxidation).$3$. Since two different elements are undergoing oxidation and reduction in different reactants,this is an intermolecular redox reaction.$4$. Therefore,the reaction is classified as an intermolecular redox reaction.

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$MnO_2 + 2NaCl + 2H_2SO_4 \longrightarrow MnSO_4 + Na_2SO_4 + 2H_2O + Cl_2 \uparrow$

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Assign $A$,$B$,$C$,$D$ from the given type of reaction.$MnO_2 + 2NaCl + 2H_2SO_4 \longrightarrow MnSO_4 + Na_2SO_4 + 2H_2O + Cl_2 \uparrow$