The theoretical density of BCC chromium is , 2.48g/cm³
ρ = [tex]\frac{N * M }{N_{A} * a^{3} }[/tex]
where
ρ = density of unit cell
a = edge length of unit cell
M = Atomic mass
Z = no. of atoms in unit cell
[tex]N_{A}[/tex] = Avogadro's number
(given)
Z = 2 (BCC)
M = 52.0 g/mol
atomic radius = 0.125 nm
edge length of unit cell is a
r = 0.866a (BCC unit cell)
a = 0.125nm/0.866 = 0.144×10⁻⁷cm
1nm = 10⁻⁷cm
using above values
ρ = 2× 52.0 / (6.022×10²³mol⁻¹ )×(0.144×10⁻⁷cm)³
ρ = 2.48g/cm³
The theoretical density of BCC chromium is , 2.48g/cm³
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