Answer:
The Number of gold atoms are =[tex]N_{Au}=1.81718*10^{22}\ atoms/cm^3[/tex]
Explanation:
The formula we are going to use is:
[tex]N_{Au}=\frac{N_A*C_{Au}}{{\frac{C_{Au}A_{Au} }{\rho_{Au}}}+\frac{A_{Au}}{\rho_{Ag}}(100-C_{Au})}[/tex]
Where:
[tex]N_{Au}[/tex] are number of gold atoms.
[tex]N_A[/tex] is Avogadro Number.
[tex]C_{Au}[/tex] is the amount of gold.
[tex]A_{Au}[/tex] is the atomic weight of gold.
[tex]\rho_{Au}[/tex] is the density of gold.
[tex]\rho_{Ag}[/tex] is the density of silver.
[tex]C_{Ag}[/tex] is the amount of silver.
[tex]N_{Au}=\frac{6.023*10^{23}*45\%wt}{\frac{45\%wt*196.97}{19.32}+\frac{196.97}{10.49}(100-45\%wt)}\\ N_{Au}=1.81718*10^{22}\ atoms/cm^3[/tex]
The Number of gold atoms are =[tex]N_{Au}=1.81718*10^{22}\ atoms/cm^3[/tex]
