Answer
The answer is 10.78 g/cm experimentally
Explanation:
Density = [tex]\frac{mass}{volume}[/tex]
We see that there BCC structure of Mo has 9 atoms, and the edge length of the cell (a) is twice the atomic radius (
r).
a = 9, r = 0.1363 nm = 1.363 A
∴ a = 2 × 9 r = 18r
Effective volume of atoms = [tex]a^{3}[/tex] =[tex](18r)^{3} = 5832(1.363)^{3}[/tex]= 14, 767.434 [tex]cm^{3}[/tex]
molar mass of Mo = 95.95 g/mol
∴Density = [tex]\frac{95.95 g/mol}{14, 767.4355 cm^{3} }[/tex] × [tex]\frac{1 mol}{6.022*10^{23} atoms Mo }[/tex]
= 1.0788 × [tex]10^{20}[/tex] = 10.79 E18
= 10.79 g/cm3 (experimental density)
Theoretical density= 10. 22 g/cm3
