Calculate the density of metal having molar mass $210 \mathrm{~g} \mathrm{~mol}^{-1}$ that forms simple…
Calculate the density of metal having molar mass $210 \mathrm{~g} \mathrm{~mol}^{-1}$ that forms simple cubic unit cell. $\left(\mathrm{a}^3 \cdot \mathrm{N}_{\mathrm{A}}=21.5 \mathrm{~cm}^3 \mathrm{~mol}^{-1}\right)$
$9.77 \mathrm{~g} \mathrm{~cm}^{-3}$
$7.15 \mathrm{~g} \mathrm{~cm}^{-3}$
$8.12 \mathrm{~g} \mathrm{~cm}^{-3}$
$6.94 \mathrm{~g} \mathrm{~cm}^{-3}$
Solution
For simple cubic unit cell, $\mathrm{n}=1$.
Density $(\rho)=\frac{\mathrm{nM}}{\mathrm{a}^3 \mathrm{~N}_{\mathrm{A}}}=\frac{1 \times 210}{21.5}=9.77 \mathrm{~g} \mathrm{~cm}^{-3}$