The amount of charge in F (Faraday) required to obtain one mole of iron from Fe 3 O 4 is ______. (Round off…

${\mathrm{Fe}}_3{\mathrm{O}}_4$ is a mixed oxide($\stackrel{+2}{\mathrm{Fe}}\mathrm{O} . {\stackrel{+3}{\mathrm{Fe}}}_2{\mathrm{O}}_3$)

The net change in oxidation can be calculated as follows,

${\mathrm{Fe}}_3{\mathrm{O}}_4\stackrel{+8{\mathrm{e}}^{-}}{⟶}3\mathrm{Fe}$

For 3 moles of formation of iron, 8 moles of electrons are involved.

One mole of electrons charge is called one Faraday.

Charge for $1$ mole $\mathrm{Fe}=\frac{8}{3}\mathrm{F}$

$=2.67 \mathrm{F}$