Answer:
1.593 grams is the mass of [tex]4.92\times 10^{21}[/tex] platinum atoms.
Explanation:
[tex]N=n\times N_A[/tex]
[tex]m=n\times M[/tex]
Where:
N = Number of particles / atoms/ molecules
n = Number of moles
m = mass of sample
M = Atomic mass
[tex]N_A=6.022\times 10^{23} mol^{-1}[/tex] = Avogadro's number
We have:
Atoms of platinum = N = [tex]4.92 \times 10^{21} [/tex]
Moles of platinum = n =?
[tex]n=\frac{N}{N_A}=\frac{4.92\times 10^{21}}{6.022\times 10^{23} mol^{-1}}[/tex]
n = 0.008170 moles
Mass of N platinum atoms = m
Atomic mass of the platinum atom = m = 195 g/mol
[tex]m=0.008170 mol\times 195 g/mol=1.593 g[/tex]
1.593 grams is the mass of [tex]4.92\times 10^{21}[/tex] platinum atoms.
