The oxidation state of chromium in the final product formed by the reaction between $KI$ and acidified potassium dichromate solution is

$A_2O_x$ is oxidised to $AO_3^-$ by $MnO_4^-$ in acidic medium. If $1.5 \times 10^{-3} \text{ mole of } A_2O_x$ requires $40 \text{ mL}$ of $0.03 \text{ M } KMnO_4$ solution in acidic medium,which of the following statement$(s)$ is/are correct?

Assign $A$,$B$,$C$,$D$ from given type of reaction.
$Zn_{(s)} + 2HCl_{(aq)} \longrightarrow ZnCl_{2(aq)} + H_{2(g)}$

The number of moles of $KMnO_4$ reduced by one mole of $KI$ in alkaline medium is

Assign $A, B, C, D$ from the given types of reactions:
$A$: Disproportionation reaction.
$B$: Comproportionation reaction.
$C$: Either intermolecular redox reaction or displacement reaction.
$D$: Either thermal combination redox reaction or thermal decomposition redox reaction.
Reaction: $MnO_4^- + H^+ + Br^- \longrightarrow Mn^{2+}(aq.) + Br_2 \uparrow$

Write the balanced chemical equation for the following reaction in an acidic medium using the ion-electron method:
Permanganate ion $(MnO_4^-)$ reacts with sulphur dioxide gas to produce $Mn^{+2}$ and hydrogen sulphate ion $(HSO_4^-)$.