Iron crystallizes as face centred cube- Its density is 2-8 g - cm 3- If the volume of the unit cell is 56-38 - 10-24 cm 3- calculate the mass of one atom-A- 39-46 - 10-24 gB- 49-46 - 10-24 gC- 2-946 - 10-24 gD- 3-946 - 10-24 g

The correct option is A 39.46 x 10 24g Density of the unit cell = 2.8 g/cm3 and volume of unit cell = 56.38 x 10 24 cm3 Mass of the unit cell = 2.8 g/cm3 x 56. ...

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Standard XII

Chemistry

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Iron crystall...

Question

Iron crystallizes as face centred cube. Its density is 2.8 g/cm³. If the volume of the unit cell is 56.38x10^-24 cm³, calculate the mass of one atom.

39.46 x 10^-24g

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49.46 x 10^-24g

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2.946 x 10^-24g

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3.946 x 10^-24g

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Solution

The correct option is A
39.46 x 10^-24g

Density of the unit cell = 2.8 g/cm³ and volume of unit cell = 56.38 x 10^-24 cm³

Mass of the unit cell = 2.8 g/cm³ x 56.38 x 10^-24 cm³

In face centred unit cell there are 4 atoms.

So mass of one atom = 2.8 g/cm³ x 56.38 x 10^-24 cm³ /4 = 39.46 x 10^-24g

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Iron crystallizes as face centred cube. Its density is 2.8 g/cm3. If the volume of the unit cell is 56.38x10-24 cm3, calculate the mass of one atom.

The correct option is A 39.46 x 10-24g Density of the unit cell = 2.8 g/cm3 and volume of unit cell = 56.38 x 10-24 cm3 Mass of the unit cell = 2.8 g/cm3 x 56.38 x 10-24 cm3 In face centred unit cell there are 4 atoms. So mass of one atom = 2.8 g/cm3 x 56.38 x 10-24 cm3 /4 = 39.46 x 10-24g

Iron crystallizes as face centred cube. Its density is 2.8 g/cm³. If the volume of the unit cell is 56.38x10^-24 cm³, calculate the mass of one atom.