A sample of ferrous oxide has actual formula `Fe_(0.93)O_(1.00)` .In this sample what fraction of metal ions are `Fe^(2+)` ions ? What type of non - stoichiometric defect is present in this sample ?

Explanation

First method:
Oxidation state (O.S) of Fe in `Fe_(0.93)O=0.93xx X-2xx1=0impliesX=2.15`
Oxidation state (O.S.) of Fe is an intermediate value of `Fe^(2+)` and `Fe^(3+)`
Let `%` of `Fe^(3+)=a`
`(3xxa+2(100-a))/(100)=2.15impliesa=15.05%`
Percent of `Fe^(3+)=15.05`