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

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:

From the given reaction:
$2 KMnO_4 + 3 H_2 SO_4 + 5 H_2 O_2 \longrightarrow K_2 SO_4 + 2 MnSO_4 + 8 H_2 O + 5 O_2$
Find the normality of $H_2 O_2$ solution,if $20 \ mL$ of it is required to react completely with $16 \ mL$ of $0.02 \ M \ KMnO_4$ solution.
$(Molar \ mass \ of \ KMnO_4 = 158 \ g \ mol^{-1})$

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:
$MnO_4^-$ : $C_2O_4^{2-}$ : $H^{+}$

Which of the following is a redox reaction?

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