The surface area is given [tex]200 inch^{2}[/tex] and thickness is 0.005 inch thus, volume will be:
[tex]V=A\times T=(200\times 0.005)inch^{3}=1inch^{3}[/tex]
Converting [tex]inch^{3}[/tex] to [tex]cm^{3}[/tex]
[tex]1 inch^{3}=16.38 cm^{3}[/tex]
The density of Nickel is [tex]8.908 g/cm^{3}[/tex] thus, mass will be:
[tex]m=d\times V=8.908 g/cm^{3}\times 16.38 cm^{3}=146 g[/tex]
Now, molar mass of nickel is 58.7 g/mol thus, number of moles can be calculated as follows:
[tex]n=\frac{m}{M}=\frac{146 g}{58.7 g/mol}=2.48 mol[/tex]
in 1 mole there are [tex]6.023\times 10^{23} atoms[/tex] thus, number of atoms in 2.48 mol will be:
[tex]N=2.48\times 6.023\times 10^{23}=1.5\times 10^{24}[/tex]
Therefore, number of atoms of nickel required is [tex]1.5\times 10^{24}[/tex]
