The reaction of aqueous $KMnO_4$ with $H_2O_2$ in acidic conditions gives

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$2NaI + MnO_2 + 2H_2SO_4 \to MnSO_4 + Na_2SO_4 + I_2 + 2H_2O$

What is the stoichiometric coefficient of the oxalate ion after balancing the following redox reaction?
$MnO_4^- + C_2O_4^{2-} + H^+ \rightarrow Mn^{2+} + CO_2 + H_2O$

The number of moles of electrons required to reduce $0.2 \ mol$ of $Cr_2O_7^{2-}$ to $Cr^{3+}$ is:

If the number of moles of $Fe^{2+}$ ions oxidized by one mole of acidified $MnO_4^{-}$ is $x$, the number of moles of $Fe^{2+}$ ions oxidized by one mole of acidified $Cr_2O_7^{2-}$ is:

In a balanced equation $H_2SO_4 + x \ HI \to H_2S + y \ I_2 + z \ H_2O$,the values of $x, y, z$ are