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(D) The reaction is: $Pb_3O_4 + 4HNO_3 \rightarrow 2Pb(NO_3)_2 + PbO_2 + 2H_2O$.In $Pb_3O_4$,the oxidation state of $Pb$ is a mixture of $+2$ and $+4$

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$D$. for either thermal combination redox reaction or thermal decomposition redox reaction.

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(D) The reaction is: $Pb_3O_4 + 4HNO_3 \rightarrow 2Pb(NO_3)_2 + PbO_2 + 2H_2O$.In $Pb_3O_4$,the oxidation state of $Pb$ is a mixture of $+2$ and $+4$ (it is $2PbO \cdot PbO_2$).When treated with dilute $HNO_3$,$PbO$ part reacts to form $Pb(NO_3)_2$ $(Pb^{2+})$,while $PbO_2$ $(Pb^{4+})$ remains as an insoluble precipitate.This is a non-redox reaction where the mixed oxide is decomposed into its constituent oxides,one of which reacts with the acid.However,in the context of standard redox classification,this reaction is often categorized as a type of disproportionation or decomposition-like process where the oxidation states do not change for the $Pb$ atoms involved in the product formation relative to their state in the mixed oxide.Given the options,$D$ is the most appropriate classification as it represents a decomposition-like redox process.

List-$I$ $(\text{Redox Reaction})$	List-$II$ $(\text{Type of Redox Reaction})$
$A$. $CH_{4(g)} + 2O_{2(g)} \xrightarrow{\Delta} CO_{2(g)} + 2H_2O_{(l)}$	$I$. Disproportionation reaction
$B$. $2NaH_{(s)} \xrightarrow{\Delta} 2Na_{(s)} + H_{2(g)}$	$II$. Combination reaction
$C$. $V_2O_{5(s)} + 5Ca_{(s)} \xrightarrow{\Delta} 2V_{(s)} + 5CaO_{(s)}$	$III$. Decomposition reaction
$D$. $2H_2O_{2(aq)} \xrightarrow{\Delta} 2H_2O_{(l)} + O_{2(g)}$	$IV$. Displacement reaction

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$Pb_3O_4 + 4HNO_3 \rightarrow 2Pb(NO_3)_2 + PbO_2 + 2H_2O$

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Assign $A$,$B$,$C$,$D$ from the given type of reaction.$Pb_3O_4 + 4HNO_3 \rightarrow 2Pb(NO_3)_2 + PbO_2 + 2H_2O$