One of the products formed due to the reaction between $KMnO_4$ and $HCl$ is

Assign $A, B, C, D$ from the given type of reaction for the following chemical equation:
$Mg_{(s)} + 2HCl_{(aq)} \longrightarrow MgCl_{2(aq)} + H_{2(g)}$

Assign $A, B, C, D$ from the given type of reaction.
$Na_2CO_3 + PbSO_4 \longrightarrow PbCO_3 \downarrow + Na_2SO_4$

$H_2O_2$ reduces $MnO_4^-$ ion to:

When chlorine gas is passed through an aqueous solution of $KBr$,the solution turns orange brown due to the formation of

Chlorine undergoes disproportionation in alkaline medium as shown below:
$a Cl_{2(g)} + b OH^{-}_{(aq)} \rightarrow c ClO^{-}_{(aq)} + d Cl^{-}_{(aq)} + e H_2O_{(l)}$
The values of $a, b, c$ and $d$ in a balanced redox reaction are respectively: