If Fe2+ and Fe3+ are present in Oxide of Iron Fe0.78O0.96 .Then Calculate Number of These Isotopes in Iron Oxide and Their % in The Iron Oxide.

Q. Iron oxide $\left({Fe}_{0.94}O\right)$ exist. What reaction of iron ions i.e. ${Fe}^{2+}$ and ${Fe}^{3+}$ present in this? Calculate their percentage.

Q. Due to metal deficiency defect, iron forms a non-stoichiometric composition in which iron is present in +2 and +3 oxidation state. In this oxide 15% iron is present in +3 oxidation state. In this oxide 15% iron is present in +3 oxidation state. The formula of oxide is:

Q. The oxidation number of iron in ${Fe}_3{O}_4$ is:

Q. $F{e}_{0.95}O$ can be due to presence of iron in $+2$ and $+3$ oxidation numbers. Then iron present in $+3$ oxidation state will be

Q. Formula of iron oxide with metal deficiency defect in its crystal is $F{e}_{0.94}O$. The crystal contains $F{e}^{2+}\text{and}F{e}^{3+}$. The mole percentage of $Fe$ existing as $F{e}^{3+}$ ion in the crystal is:
[0.77 Mark]