Question

One mole of iron [$55.8$gm], when oxidised to $+2$ oxidation states gives up:

• A. 1 $N_A$ electron
• B. 2 $N_A$ electron
• C. 3 $N_A$ electron
• D. 0.5 mole of electron

Answer 1

The correct option is B 2 $N_A$ electron

The oxidation reaction of $Fe$ to $F{e}^{2+}$ can be written as

$Fe⟶F{e}^{2+}+2e^{-}$

$1mol$ $1mol$ $2mol$

From the reaction, it is evident that, one mole of $Fe$ gives two moles electrons on oxidation to$F{e}^{2+}$.

We know that, $1mol=N_A$

$2mol$ of electrons$=2N_A$

$1molFe$ releases $2N_A$ electrons on oxidation to$F{e}^{2+}$.