Given below are two statements:Statement-I : | vedclass

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(D) In Statement-$I$, heating $NaCl$ with $H_2SO_4$ and $MnO_2$ produces $Cl_2$ gas. The reaction is: $MnO_2 + 2NaCl + 2H_2SO_4 \rightarrow MnSO_4 + N

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Statement-$I$ is incorrect but Statement-$II$ is correct.

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(D) In Statement-$I$, heating $NaCl$ with $H_2SO_4$ and $MnO_2$ produces $Cl_2$ gas. The reaction is: $MnO_2 + 2NaCl + 2H_2SO_4 \rightarrow MnSO_4 + Na_2SO_4 + 2H_2O + Cl_2$. Here, the oxidation state of $Mn$ changes from $+4$ in $MnO_2$ to $+2$ in $MnSO_4$, which is a reduction process, not oxidation. Thus, Statement-$I$ is incorrect.In Statement-$II$, heating $NaI$ with $H_2SO_4$ and $MnO_2$ also produces $I_2$ gas. The reaction is: $MnO_2 + 2NaI + 2H_2SO_4 \rightarrow MnSO_4 + Na_2SO_4 + 2H_2O + I_2$. Here, the oxidation state of $Mn$ changes from $+4$ in $MnO_2$ to $+2$ in $MnSO_4$, which is a reduction process. Thus, Statement-$II$ is correct.

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

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