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

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

The equivalent weight of ${S_2O_3^{2-}}$ in the reaction where it acts as a reductant is ...... . ${2S_2O_3^{2-} + I_2 \rightarrow S_4O_6^{2-} + 2I^-}$

In the balanced reaction $xBrO_3^- + yCr^{3+} + zH_2O \to aBr_2 + bHCrO_4^- + cH^+$,the coefficients $x, y$ and $z$ are

In the reaction $I_2 + 2S_2O_3^{2-} \to 2I^{-} + S_4O_6^{2-}$,the equivalent weight of iodine will be equal to

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: