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Q.
The number of moles of $KMnO_{4}$ that will be needed to react completely with one mole of ferrous oxalate in acidic solution is
AMUAMU 2001
Solution:
When $KMnO _{4}$ reacts with ferrous oxalate in acidic solution then the following reaction takes place.
$\overset{+7}{Mn} O _{4}^{-}+ \overset{+2}{Fe}\overset{+3}{C _{2}} O _{4} \longrightarrow \overset{+2}{Mn ^{+2}}+\overset{+4}{2 CO _{2}}+ Fe ^{3+}$
Here, $Mn ^{7+}$ is reduced to $Mn ^{2+}(+7 \rightarrow+2)$ and carbon is oxidised to $CO _{2}(+3 \rightarrow+4)$ and $Fe ^{2+}$ is oxidised to $Fe ^{3+}(+2 \rightarrow+3)$. Thus,
Reduction $Mn ^{7+}+5 e^{-} \longrightarrow Mn ^{2+} \downarrow 5$
The balanced chemical equation is as
$\because 5$ moles of $FeC _{2} O _{4}$ are oxidised by 3 moles of $KMnO _{4}$.
$\therefore 1$ mole of $FeC _{2} O _{4}$ is oxidised by $\frac{3}{5}$ moles of $KMnO _{4}$.
