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

What is the value of $x$ in order to balance the following redox reaction by the ion-electron method?
$x H_2O_2 + ClO_4^{-} \rightarrow x O_2 + ClO_2^{-} + 2 H_2O$

$ClO_2$ oxidizes $H_2O_2$ to $O_2$ in basic medium and is itself reduced to $Cl^-$. How many moles of $H_2O_2$ will be oxidized by one mole of $ClO_2$ (in $.5$)?

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

In the reaction $X^- + XO_3^- + H^+ \longrightarrow X_2 + H_2O$,the molar ratio in which $X^-$ and $XO_3^-$ react 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?