The number of $F e^{2 +}$ ion oxidised by one mole of ${M n O}_{4}^{-}$ ions is :

\frac{1}{5}

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\frac{2}{3}

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5

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\frac{3}{2}

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Solution

The correct option is A $5$
Reaction:
$F e^{+ 2} + K M n O_{4} \to M n^{+ 2} + F e^{+ 3}$
+2 +7 +2 +3
So, one mole of $K M n O_{4}$ oxidises $5$ mole of ferrous ion.

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Q. A given amount of

{F e}^{2 +}

is oxidised by

x

moles of

M n O_{4}^{-}

in acidic medium. Calculate number of moles of

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{F e}^{2 +}

in acidic medium if

x = 5

When the ion ${C r}_{2} O_{7}^{2 -}$ acts as an oxidant in acidic aqueous solution the ion ${C r}^{3 +}$ is formed. How many moles of ${S n}^{2 +}$ would be oxidised to ${S n}^{4 +}$ by one mole of ${C r}_{2} O_{7}^{2 -}$ ions?

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The number of Fe2+ ion oxidised by one mole of MnO−4 ions is :

The correct option is A 5Reaction:Fe+2+KMnO4→Mn+2+Fe+3 +2 +7 +2 +3 So, one mole of KMnO4 oxidises 5 mole of ferrous ion.

The number of $F e^{2 +}$ ion oxidised by one mole of ${M n O}_{4}^{-}$ ions is :

The correct option is A $5$
Reaction:
$F e^{+ 2} + K M n O_{4} \to M n^{+ 2} + F e^{+ 3}$
+2 +7 +2 +3
So, one mole of $K M n O_{4}$ oxidises $5$ mole of ferrous ion.