Assign $A, B, C, D$ from the given type of reaction.
$Na_2SO_3 + BaCl_2 \longrightarrow BaSO_3 \downarrow + 2NaCl$

$A$ sample $(5.6 \ g)$ containing iron is completely dissolved in cold dilute $HCl$ to prepare $250 \ mL$ of solution. Titration of $25.0 \ mL$ of this solution requires $12.5 \ mL$ of $0.03 \ M \ KMnO_4$ solution to reach the end point. The number of moles of $Fe^{2+}$ present in the $250 \ mL$ solution is $x \times 10^{-2}$ (consider complete dissolution of $FeCl_2$). The amount of iron present in the sample is $y \%$ by weight. (Assume: $KMnO_4$ reacts only with $Fe^{2+}$ in the solution. Use: Molar mass of iron as $56 \ g \ mol^{-1}$)
$(1)$ The value of $x$ is. . . . .
$(2)$ The value of $y$ is. . . . .

Match the chemical reactions given in List-$I$ with their types given in List-$II$:

List-$I$	List-$II$
$A$. $TiCl_{4(l)} + 2Mg_{(s)} \xrightarrow{\Delta} Ti_{(s)} + 2MgCl_{2(s)}$	$I$. Disproportionation reaction
$B$. $2H_2O_{2(aq)} \rightarrow 2H_2O_{(l)} + O_{2(g)}$	$II$. Metal displacement reaction
$C$. $C_{(s)} + O_{2(g)} \xrightarrow{\Delta} CO_{2(g)}$	$III$. Decomposition reaction
$D$. $2NaH_{(s)} \xrightarrow{\Delta} 2Na_{(s)} + H_{2(g)}$	$IV$. Combination reaction

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

Identify the substance acting as an oxidant in the following reaction:
$BaCl_2 + Na_2SO_4 \to BaSO_4 + 2NaCl$

Consider the following reactions (unbalanced):
$Zn +$ hot conc. $H_2SO_4 \rightarrow G + R + X$
$Zn +$ conc. $NaOH \rightarrow T + Q$
$G + H_2S + NH_4OH \rightarrow Z$ (a precipitate) $+ X + Y$
Choose the correct option$(s)$.
$(1)$ The oxidation state of $Zn$ in $T$ is $+1$
$(2)$ Bond order of $Q$ is $1$ in its ground state
$(3)$ $Z$ is dirty white in colour
$(4)$ $R$ is a $V$-shaped molecule