In an alkaline solution,$ClO_2$ oxidizes $H_2O_2$ to $O_2$ and is itself reduced to $Cl^-$. How many moles of $H_2O_2$ will be oxidized by $1 \ mol$ of $ClO_2$?

In an alkaline medium,$ClO_2$ oxidizes $H_2O_2$ to $O_2$ and is reduced to $Cl^-$. How many moles of $H_2O_2$ will be oxidized by $1$ mole of $ClO_2$?

In the reduction of dichromate by $Fe(II)$,the number of electrons involved per chromium atom is:

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$Cl_{2(g)} + 2KI(aq.) \longrightarrow 2KCl(aq.) + I_2(s)$

The values of coefficients to balance the following reaction are
$Cr(OH)_3 + ClO^{-} + OH^{-} \to CrO_4^{2-} + Cl^{-} + H_2O$
Find the coefficients for $Cr(OH)_3$,$ClO^{-}$,$CrO_4^{2-}$,and $Cl^{-}$ respectively.

Write the net ionic equation for the reaction of potassium dichromate$(VI)$,$K_{2}Cr_{2}O_{7}$ with sodium sulphite,$Na_{2}SO_{3}$ in an acidic solution to give chromium$(III)$ ion and the sulphate ion.