Question

Number of moles of ${Mn{O}_4}^{-}$ required to oxidize one mole of ferrous oxalate completely in the acidic medium will be:

• A. $7.5moles$
• B. $0.2moles$
• C. $0.6moles$
• D. $0.4moles$

Answer 1

Answer: (C)

$0.6moles$

The balanced chemical reaction is-

$3{Mn{O}_4}^{-}+5Fe{C}_2{O}_4+24H^{+}⟶3{Mn}^{2+}+5{Fe}^{+3}+10C{O}_2+12H_{2}O$

As shown in the above reaction,

No. of moles of ${Mn{O}_4}^{-}$ required to oxidize 5 moles of ferrous oxalate $=3\text{moles}$

$\therefore$ No. of moles of ${Mn{O}_4}^{-}$ required to oxidize 1 mole of ferrous oxalate $=\frac{3}{5}=0.6\text{moles}$.

Hence, the correct option is $D$.