Calculate the density of a metal with molar mass $56 \ g \ mol^{-1}$ that crystallises in a $bcc$ structure with an edge length of $288 \ pm$. (in $g \ cm^{-3}$)

The density of $Na$ is $0.613 \ g \ cm^{-3}$. If the edge length of the unit cell of $Na$ is $5 \ \mathring{A}$,the effective number of atoms of $Na$ per unit cell is (Atomic weight of $Na = 23 \ u$)

If the density of a $CsCl$ crystal,which crystallizes in a $bcc$ structure,is $3.988 \, g/cm^3$,then the edge length of the unit cell will be ........ $(CsCl = 168.4 \, g/mol)$.

What is the atomic radius of polonium if it crystallises in a simple cubic structure with edge length of unit cell $336 \ pm$ (in $pm$)?

For a crystal,the angle of diffraction $(2 \theta)$ is $90^{\circ}$ and the second order line has a $d$ value of $2.28 \ \text{Å}$. The wavelength (in $\text{Å}$) of $X$-rays used for Bragg's diffraction is

Which of the following instruments is used to determine the crystal structure?