Number of moles of ferrous sulphate oxidised by 1 mole of potassium permanganate in acidic medium is:

\frac{2}{5}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

\frac{5}{2}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

\frac{1}{5}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

5

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct option is D $5$
The reaction between Ferrous sulphate & potassium permanganate is given as :
${2 K M n O}_{4} + {8 H}_{2} {S O}_{4} + 10 {F e S O}_{4} \to K_{2} {S O}_{4} + {2 M n S O}_{4} + 8 H_{2} O + 5 F e {({S O}_{4})}_{3}$
Therefore, by stiochiometry,
$2$ moles of ${K M n O}_{4} \equiv 10$ moles of ${F e S O}_{4}$
Therefore, $1$ mole of ${K M n O}_{4} \equiv 5$ moles of ${F e S O}_{4}$
Therefore, $5$ moles of ferrous sulphate are oxidized by $1$ mole of potassium permanganate in acidic medium.

Suggest Corrections

Similar questions

K M n O_{4}

m o l e s

p e r m o l e

m o l e s

K M n O_{4}

p e r m o l e

{F e}^{2 +}

x

M n O_{4}^{-}

{C r}_{2} O_{7}^{2 -}

{F e}^{2 +}

x = 5

Join BYJU'S Learning Program