Question

The number of moles of acidified $KMn{O}_4$ required to oxidize one mole of ferrous oxalate, $Fe{C}_2{O}_4$ is:

• A. 5
• B. 3
• C. 0.6
• D. 1

Answer 1

The correct option is C 0.6

The balanced chemical reaction between ${KMnO}_4$ and ${FeC}_2{O}_4$ is

${3KMnO}_4+5Fe{C}_2{O}_4+2{4H}^{+}⟶{5Fe}^{+3}+10{CO}_2+3{Mn}^{+2}+3K^{+}$

$5$ moles of ${FeC}_2{O}_4$ reacts with $3$ moles of ${KMnO}_4$

then $1$ mole $\to$ $x$ moles

$x=\frac{3}{5}=0.6$

Ans :- Option C.