Answer:
8.5 × 10²² atom / cm³, 2.125 × 10²² unit cells / cm³, 4.7 × 10⁻²³ cm³ / cell unit, 3.61 × 10⁻⁸ cm /cell
Explanation:
The density of the solid Cu = 8.96 g/cm³
a) number of atoms present
mole = mass / molar mass = (8.96 g/cm³) / 63.546 = 0.141 mol
number of atoms = mole × avogadro's constant = 0.141 × 6.02 × 10²³ = 8.5 × 10²² atom / cm³
b) a face-centered cubic unit cell contains 4 atoms
8.5 × 10²² atom / cm³ / 4 = 2.125 × 10²² unit cells / cm³
c) the volume of a unit cell of the metal = reciprocal of 2.125 × 10²² unit cells / cm³ = 1 ÷ ( 2.125 × 10²² unit cells / cm³ ) = 4.7 × 10⁻²³ cm³ / cell unit
the edge length of a cell of cu = ∛(4.7 × 10⁻²³ cm³ / cell unit) = 3.61 × 10⁻⁸ cm /cell
