The substance $CuCl$ has a $ZnS$ $(ccp)$ structure. If its density is $3.4 \ g \ cm^{-3}$, what is the edge length of the unit cell?

The formula for the determination of the density of a unit cell is:

$A$ metal has a $fcc$ lattice. The edge length of the unit cell is $404 \, pm$. The density of the metal is $2.72 \, g \, cm^{-3}$. The molar mass of the metal is :- ............ $g \, mol^{-1}$ ( $N_A$ Avogadro constant $= 6.02 \times 10^{23} \, mol^{-1}$ )

$KBr$ has $NaCl$ structure. Its density is $2.75 \ g \ cm^{-3}$. The edge length of the unit cell will be (molar mass of $KBr$ is $119 \ g \ mol^{-1}$):

Tobacco seed globin forms face-centered cubic crystals with a unit cell dimension of $12.3 \, nm$ and a density of $1.287 \, g \, cm^{-3}$. Its molecular mass will be:

Calculate the radius of a metal atom if it forms a $bcc$ unit cell having an edge length of $530 \ pm$. (in $pm$)