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Ferrous oxide has a cubic structure and ...

Ferrous oxide has a cubic structure and each dege of the unit cell is 5.0 Å. Assuming density of the oxide as `"4.0 g cm"^(-3)` then the number of `Fe^(2+)` and `O^(2-)` ions present in each unit cell will be

Text Solution

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Volume of the unit cell `= (5xx10^(-8)cm)^(3)=1.25xx10^(-22)cm^(3)`
Density of `FeO = 4 g cm^(-3)`
Therefore, mass of unit cell `= 1.25xx10^(-22)xx4=5xx10^(-22)g`
Mass of one molecule of FeO = Molar mass in g/ Avogadro.s number
`= (72 g mol^(-1))/(6.022xx10^(23)mol^(-1))=1.195xx10^(-22)g`.
Number of FeO molecules per unit cell `= (5xx10^(-22))/(1.195xx10^(-22))~~4`
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