One mole of potassium dichromate completely oxidises the following number of moles of ferrous sulphate in acidic medium.

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

What is the value of $x$ in order to balance the following redox reaction?
$Mn_{(aq)}^{2+} + x ClO_{3_{(aq)}}^{-} \rightarrow MnO_{2_{(s)}} + x ClO_{2_{(aq)}}$

What is the number of electrons gained by $Cl$ atom when $n$ mole of $ClO_4^-$ is transformed into $n$ mole of $ClO_2^-$ ion?

For the balanced equation $NO_2^- + H_2O \to NO_3^- + 2H^+ + ne^-$,the value of $n$ is .......

$KMnO_4$ oxidises oxalic acid to $CO_2$ in acidic medium. The equivalent weight of $KMnO_4$ is $(Mn = 55, K = 39, O = 16)$: