Gold forms a substitutional solid solution with silver. Compute the number of gold atoms per cubic centimeter for a silver-gold alloy that contains 42 wt% Au and 58 wt% Ag. The densities of pure gold and silver are 19.32 and 10.49 g/cm3, respectively. The atomic weight of Au is 196.97 g/mol.

The number of gold atoms per cubic centimeters in the given alloy is

Explanation:

To calculate the number of gold atoms per cubic centimeters for te given silver-gold alloy, we use the equation:

where,

= number of gold atoms per cubic centimeters

= Avogadro's number =

= Mass percent of gold in the alloy = 42 %

= Density of pure gold =

= Density of pure silver =

= molar mass of gold = 196.97 g/mol

Putting values in above equation, we get:

Hence, the number of gold atoms per cubic centimeters in the given alloy is

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number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.