Answer:
[tex]V_{c}=1.396x10^{-28} m^{3} /unit.cell[/tex]
Explanation:
z = number of atoms
M = Molar mass of zirconium
N = Avogadro’s number
Vc = volume of zirconium unit cell
d = density
[tex]z=12x\frac{1}{6}+2x\frac{1}{2}+3=6[/tex]
z = 6 atoms per unit cell
M = 91.224 g/mol
N = [tex]6.023x10^{23} atoms/mol[/tex]
d = [tex]6.51g/cm^{3}[/tex]
[tex]V_{c}=\frac{zxM}{dxN}[/tex]
[tex]V_{c}=\frac{6x(91.224g/mol)}{(6.51g/cm^{3}) x(6.023x10^{23}atoms/mol) }[/tex]
[tex]V_{c}=1.396x10^{-22} cm^{3} /unit.cell[/tex]
[tex]V_{c}=1.396x10^{-28} m^{3} /unit.cell[/tex]
