Silver forms a $CCP$ structure and its density is $10.5 \ g/cm^3$. What is the edge length of the unit cell? (Molar mass of silver is $107.9 \ g/mol$)

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 $Na = 23 \ u$)

Calculate the number of unit cells in $1 \ cm^3$ of an element if the unit cell edge length is $2.0 \times 10^{-8} \ cm$.

At $T \ K$, copper (atomic mass $= 63.5 \ u$) has $fcc$ structure with an edge length of $x \ \mathring{A}$. The density of copper (in $g \ cm^{-3}$) at that temperature is approximately $(N_A = 6.0 \times 10^{23} \ mol^{-1})$

How many unit cells are present in $100 \ g$ of an element with $fcc$ crystal structure having density $10 \ g/cm^{3}$ and edge length $100 \ pm$?

When silver crystallizes, it forms face-centered cubic $(FCC)$ unit cells. If the volume of the unit cell is $6.84 \times 10^{-23} \text{ cm}^3$, calculate the density of silver. (Molar mass of silver is $108 \text{ g/mol}$, $N_A = 6.022 \times 10^{23} \text{ mol}^{-1}$) (in $\text{ g cm}^{-3}$)