$ClO_2$ 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 $.5$)?

When sulphur dioxide is passed in an acidified $K_{2}Cr_{2}O_{7}$ solution,the oxidation state of sulphur is changed from

Assign $A, B, C, D$ from the given type of reaction.
$Fe^{2+}(aq.) + Cr_2O_7^{2-}(aq.) + H^+(aq.) \longrightarrow Fe^{3+}(aq.) + Cr^{3+}(aq.) + H_2O(l)$

The oxidation state of chromium in the final product formed in the reaction between $KI$ and acidified $K_{2}Cr_{2}O_{7}$ solution is:

In the half-reaction $Cr_2O_7^{2-} + 14H^+ + 6e^- \rightarrow 2Cr^{3+} + 7H_2O$,the equivalent weight of $Cr_2O_7^{2-}$ is obtained by dividing its molecular weight by:

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.