Calculate the density of a metal having a molar mass of $210 \ g \ mol^{-1}$ that forms a simple cubic unit cell. $(a^3 \cdot N_{A} = 21.5 \ cm^3 \ mol^{-1})$ (in $g \ cm^{-3}$)

An element crystallises in a $fcc$ lattice with cell edge $250 \ pm$. Calculate the density of the element (atomic mass $= 90.3 \ g \ mol^{-1}$) (in $g \ cm^{-3}$)

Salt $AB$ has a zinc blende structure. The radii of $A^{2+}$ and $B^{2-}$ ions are $0.7 \ \mathring{A}$ and $1.8 \ \mathring{A}$ respectively. The edge length of the $AB$ unit cell is ........... $\mathring{A}$.

What is the number of unit cells present in $3.9 \ g$ of potassium if it crystallizes in $BCC$ structure?

At $100\, ^\circ C$,copper $(Cu)$ has $FCC$ unit cell structure with cell edge length $x\, \mathring{A}$. What is the approximate density of $Cu$ (in $g\, cm^{-3}$) at this temperature? [Atomic mass of $Cu = 63.55\, u$]

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 $g \ cm^{-3}$)