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

The volume of $0.02 \ M$ acidified acidified permanganate solution required for complete reaction of $60 \ mL$ of $0.01 \ M \ I^{-}$ ion solution to form $I_2$ in $mL$ is

Find the values of $x$ and $y$ for the following balanced equation:
$xCl_2 + 6OH^- \to ClO_3^- + yCl^- + 3H_2O$

Treatment of alkaline $KMnO_{4}$ solution with $KI$ solution oxidises iodide to:

Permanganate $(VII)$ ion,$MnO_4^-$,in basic solution oxidises iodide ion,$I^-$,to produce molecular iodine $(I_2)$ and manganese $(IV)$ oxide $(MnO_2)$. Write a balanced ionic equation to represent this redox reaction.

Assign $A, B, C, D$ from the given type of reaction for the following chemical equation:
$3Fe_{(s)} + 4H_2O_{(g)} \xrightarrow{\Delta} Fe_3O_{4(s)} + 4H_{2(g)}$