In the reaction $2[Fe(CN)_6]^{3-} + H_2O_2 + 2OH^{-} \rightarrow 2[Fe(CN)_6]^{4-} + 2H_2O + O_2$,what is the equivalent weight of the reductant? $(Fe = 56, C = 12, N = 14, O = 16, H = 1)$

In neutral medium,potassium permanganate oxidises $I^{-}$ to $X$. Identify $X$.

How many electrons are lost in the following transformation?
$3Fe + 4H_2O \to Fe_3O_4 + 4H_2$

Choose the correct option regarding the reaction $2KClO_3 \to 2KCl + 3O_2$.
$(1)$ $KClO_3$ undergoes both oxidation and reduction.
$(2)$ $Cl^{+5}$ is converted to $Cl^{-}$.
$(3)$ Oxygen in $KClO_3$ undergoes reduction.
$(4)$ This reaction cannot be called a redox reaction.

In neutral or faintly alkaline medium,$KMnO_4$ being a powerful oxidant can oxidize thiosulphate almost quantitatively to sulphate. In this reaction,the overall change in the oxidation state of manganese will be:

For the redox reaction $MnO_4^- + C_2O_4^{2-} + H^{+} \to Mn^{2+} + CO_2 + H_2O$,the correct coefficients of the reactants for the balanced reaction are:
$MnO_4^-$ : $C_2O_4^{2-}$ : $H^{+}$