Answer:
[tex]\large\boxed{\large\boxed{5.00\times 10^{22}atoms/cm^3}}[/tex]
Explanation:
You can convert the density into atomic density using the atomic weight and Avogadro's number
A dimensional analysis is very helpful:
[tex]\dfrac{g}{cm^3}\times \dfrac{mol}{g}\times \dfrac{atoms}{mol}=\dfrac{atoms}{cm^3}[/tex]
Follow the chain: g cancels with g, mol cancels with mol; at the end, what remains is atoms/cm³, which is what you want.
Use that with your data:
[tex]\dfrac{2.33g}{cm^3}\times \dfrac{1mol}{28.09g}\times \dfrac{6.022\times 10^{23}atoms}{mol}=\approx 5.00\times10^{22}atoms/cm^3[/tex]
