Question

The number of moles of ${\mathrm{MnO}}_4^{-}$ required to oxidize one mole of ferrous oxalate completely in an acidic medium will be:

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

Answer 1

The correct option is A

0.6 moles

Explanation for correct answer:-

Option (A) 0.6 moles.

Step 1: Writing the reaction

$5{\mathrm{FeC}}_2{\mathrm{O}}_4+3{\mathrm{MnO}}_4^{-}+24{\mathrm{H}}^{+}\to 5{\mathrm{Fe}}^{3+}+10{\mathrm{CO}}_2+3{\mathrm{Mn}}^{2+}+12{\mathrm{H}}_2\mathrm{O}$

Step 2: Calculating the molar equivalence

15 electrons are being exchanged between 5 moles of ferrous oxalate and 3 moles of permanganate ion.

So, one mole of ferrous oxalate reduced $\frac{3}{5}\mathrm{moles}$ of permanganate ion.

Therefore, $0.6mole$of permanganate ion will oxidize one mole of ferrous oxalate completely in an acidic environment.

Hence option A is correct.