Iron crystallizes in a body-centered cubic unit. The edge of this cell is 287 pm. Calculate the density of iron
As we Know
Density = Mass/ Volume.
Therefore here
Mass is calculated for BCC unit cell i.e. for 2 atom.
Mass of One Atom = molar mass/ avogadro number.
= 55.845/6.023×10^23
=9.2720 × 10^-23 gram
Therefore for 2 atom I.e. for BCC unit cell
= 18.5440 × 10^-23 gram
Now volume = (edge)^3 I.e. (a)^3
Edge length =a= 287 pm = 287 ×10^-10 cm
a^3= (287×10^-10)^3
Volume =a^3=2.3640 × 10^-23 cm^3
Now density = Mass/ Volume
= (18.5440× 10^-23)/(2.3640×10^-23)
= 7.8443 gram / cm^3
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