Density of Unit Cells

Calcium crystallizes in a face centred cubic unit cell with a $\text{=}\text{0}\text{.560}\text{nm}\text{.}$  The density of the metal if it contains 0.1% schottky defects would be:

Copper crystallises in a face-centred cubic lattice and has a density of  $8.930\mathrm{g}{\mathrm{cm}}^{-3}$ at $393 \mathrm{K}.$ The radius of a copper atom is:
[Atomic mass of$\mathrm{Cu}=63.55\mathrm{u},{\mathrm{N}}_{\mathrm{A}}=6.02\times {10}^{23}{\mathrm{mol}}^{-1}]$

Iron has a body-centered cubic unit cell of cell edge $286.65 \mathrm{pm}$. The density of iron is $7.87 \mathrm{g} {\mathrm{cm}}^{-3}$. The Avogadro number is

(Atomic mass of iron $=56\hspace{0.17em}\mathrm{g}\hspace{0.17em}{\mathrm{mol}}^{-1}$)

X-rays diffraction studies show that copper crystallizes in an FCC unit cell with cell edge of  $3.6885\times {10}^{-8}\mathrm{cm}.$ In a separate experiment, copper is determined to have a density of  $\text{8}{\text{.92g/cm}}^{\text{3}}$, the atomic mass of copper would be:

In face-centred cubic $\left(\mathrm{FCC}\right)$ and body centred cubic $\left(\mathrm{BCC}\right),$ whose unit cell lengths are $3.5$ and $3.0$ $\mathrm{\AA }$ respectively, a metal crystallises into two cubic phases. What is the ratio of densities of $\mathrm{FCC}$ and $\mathrm{BCC}?$

The density of mercury is 13.6 g ml^-1. The approximate diameter of an atom of mercury assuming that each atom is occupying a cube of edge length equal to the diameter of the mercury atom is

An atomic substance A of molar mass $12 \mathrm{g} {\mathrm{mol}}^{–1}$has a cubic crystal structure with edge length of $300\mathit{ }\mathrm{pm}$. The no. of atoms present in one unit cell of A is

(Nearest integer)

Given the density of A is $3.0 \mathrm{g} \mathrm{m} {\mathrm{m}}^{-1}$ and ${\mathrm{N}}_{\mathrm{A}}=6.02\times {10}^{23} {\mathrm{mol}}^{-1}$

The edge length of bcc type of unit cell of metal having molecular weight $75 \mathrm{g}/\mathrm{mol}$is $5 {\mathrm{A}}^{\mathrm{o}}$. What is the radius of metal atom if its density is $2 \mathrm{g}/\mathrm{cc}$?

Find the number of atoms per unit cell if edge length is $300 \mathrm{pm}$, density$= 3 \mathrm{g}/{\mathrm{cm}}^3$, molecular mass $= 40 \mathrm{g}$ ( nearest integer)

The edge length of $\mathrm{NaCl}$ unit cell is $654 \mathrm{pm}$. What is the density of the unit cell?

The density of iridium is $22.4\mathrm{g}/{\mathrm{cm}}^3$. The unit cell of iridium is fcc. Calculate the radius of iridium atom. Molar mass of iridium is $192.2\mathrm{g}/\mathrm{mol}.\left(136\mathrm{pm}\right)$.

$\mathrm{Cu}$ metal crystallises in face centred cubic lattice with cell edge, $\mathrm{a}= 361.6 \mathrm{pm}$. What is the density of $\mathrm{Cu}$ crystal ?$\left(\mathrm{Atomic} \mathrm{mass} \mathrm{of} \mathrm{Cu}=63.5 \mathrm{amu}, {\mathrm{N}}_{\mathrm{A}}=6.023\times {10}^{23}\right)$

Gold occurs as face centred cube and it has a density of $19.30 \mathrm{kg} {\mathrm{dm}}^{-3}.$ Calculate atomic radius of gold. (Molar mass of $\mathrm{Au}=197$)

An fcc lattice has lattice parameter $\mathrm{a}= 400 \mathrm{pm}$. Calculate the molar volume of the lattice including the empty space

The density of nickel (face centred cubic cell) is $8.94 \mathrm{g}/{\mathrm{cm}}^3 \mathrm{at} 20°\mathrm{C}.$ What is the radius of the atom? (Atomic mass of $\mathrm{Ni}=59$)

Vacant space in body centered cubic lattice unit cell is about

Iron crystalizes in $\mathrm{FCC}$ with an edge length of $400\mathrm{pm}$. If it contains $0.1\%$ Schottky defects, calculate its approximate density [$\mathrm{AW}$ of $\mathrm{Fe}=56 \mathrm{g}/\mathrm{mol}$]

Metallic iron crystallizes in $\mathrm{BCC}$ at room temperature and transforms to $\mathrm{FCC}$ structure at high temperature. Calculate the ratio of density of iron at low temperature to that of high temperature [$\mathrm{MW}$ and radius of iron atom remained constant]

Atom $\mathrm{X}$ occupies the fcc lattice sites as well as alternate tetrahedral voids of the same lattice. The packing efficiency (in $\%$) of the resultant solid is closest to