Calculate the equivalent mass of each oxidant and reductant in:

${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3+{\mathrm{I}}_2⟶{\mathrm{Na}}_2{\mathrm{S}}_4{\mathrm{O}}_6+2\mathrm{NaI}$

Calculate the equivalent mass of each oxidant and reductant in:

${\mathrm{FeC}}_2{\mathrm{O}}_4⟶{\mathrm{Fe}}^{3+}+{\mathrm{CO}}_2$

Stannous ion is oxidised by the dichromate ion in acidic solution as $3{\mathrm{Sn}}^{2+}+14{\mathrm{H}}^{+}+{\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}⟶3{\mathrm{Sn}}^{4+}+2{\mathrm{Cr}}^{3+}+7{\mathrm{H}}_2\mathrm{O}$

If, $Sn{\mathrm{Cl}}_2$ is the source of ${\mathrm{Sn}}^{2+},$ how many grams of ${\mathrm{SnCl}}_2$ would be contained in $2 \mathrm{litres}$ of $0.1$ $\mathrm{N}$ solution?

The dichromate ion in an acidic solution oxidizes stannous ion as,
$3{\mathrm{Sn}}^{2+}+14{\mathrm{H}}^{+}+{\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}⟶3{\mathrm{Sn}}^{4+}+2{\mathrm{Cr}}^{3+}+7{\mathrm{H}}_2\mathrm{O}$

If ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ is source of ${\mathrm{Cr}}_2{\mathrm{O}}_7^{2-},$ what is the normality of solution containing $4.9 \mathrm{g} {\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ in $0.1$$\mathrm{litre}$ of solution?

Equivalent mass of ${\mathrm{Fe}}_3{\mathrm{O}}_4$ and ${\mathrm{Fe}}_2{\mathrm{O}}_3$ in the change ${\mathrm{Fe}}_3{\mathrm{O}}_4$ $⟶{\mathrm{Fe}}_2{\mathrm{O}}_3$ are

 (${\mathrm{M}}_1$ and ${\mathrm{M}}_2$ are molar mass of  ${\mathrm{Fe}}_3{\mathrm{O}}_4$ and ${\mathrm{Fe}}_2{\mathrm{O}}_3$, respectively.)

Find out how many moles of ${\mathrm{KMnO}}_4$ are needed to oxidise a mixture of $1 \mathrm{mole}$ each of ${\mathrm{FeSO}}_4, {\mathrm{FeC}}_2{\mathrm{O}}_4$ and ${\mathrm{Fe}}_2\left({\mathrm{C}}_2{\mathrm{O}}_4\right)$ completely in each medium?