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(D) $SO_2$ acts as a reducing agent in the presence of moisture.$(I)$ $SO_2$ reduces $O_3$ to $O_2$: $SO_2 + O_3 	o SO_3 + O_2$.$(II)$ $SO_2$ reduces

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$I, II, III$

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(D) $SO_2$ acts as a reducing agent in the presence of moisture.$(I)$ $SO_2$ reduces $O_3$ to $O_2$: $SO_2 + O_3 	o SO_3 + O_2$.$(II)$ $SO_2$ reduces acidic dichromate $(Cr_2O_7^{2-})$ to $Cr^{3+}$: $Cr_2O_7^{2-} + 3SO_2 + 2H^{+} 	o 2Cr^{3+} + 3SO_4^{2-} + H_2O$.$(III)$ $SO_2$ reduces acidic permanganate $(MnO_4^{-})$ to $Mn^{2+}$: $2MnO_4^{-} + 5SO_2 + 2H_2O 	o 2Mn^{2+} + 5SO_4^{2-} + 4H^{+}$.$(IV)$ $SO_2$ acts as an oxidizing agent towards $H_2S$: $SO_2 + 2H_2S 	o 3S + 2H_2O$. Thus,$H_2S$ is oxidized,not reduced.Therefore,$SO_2$ reduces $O_3$,$Cr_2O_7^{2-}$,and $MnO_4^{-}$. The correct option is $D$.

List-$I$ (Types of redox reactions)	List-$II$ (Examples)
$a.$ Combination reaction	$(i)$ $Cl_{2(g)} + 2Br^-_{(aq)} \rightarrow 2Cl^-_{(aq)} + Br_{2(l)}$
$b.$ Decomposition reaction	$(ii)$ $2H_2O_{2(aq)} \rightarrow 2H_2O_{(l)} + O_{2(g)}$
$c.$ Displacement reaction	$(iii)$ $CH_{4(g)} + 2O_{2(g)} \xrightarrow{\Delta} CO_{2(g)} + 2H_2O_{(l)}$
$d.$ Disproportionation reaction	$(iv)$ $2H_2O_{(l)} \xrightarrow{\text{electrolysis}} 2H_{2(g)} + O_{2(g)}$

Which of the following reactants can be reduced by $SO_2$ in the given reactions?
$(I)$ $O_3 \to$ product
$(II)$ $Cr_2O_7^{2-} \xrightarrow{H^{+}} $ product
$(III)$ $MnO_4^{-} \xrightarrow{H^{+}} $ product
$(IV)$ $H_2S \to$ product

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Which of the following reactants can be reduced by $SO_2$ in the given reactions?$(I)$ $O_3 \to$ product$(II)$ $Cr_2O_7^{2-} \xrightarrow{H^{+}} $ product$(III)$ $MnO_4^{-} \xrightarrow{H^{+}} $ product$(IV)$ $H_2S \to$ product