Answer: [tex](2.68\times 10^{11}atoms Ag/6.02\times 10^{23}atoms Ag)(107.88 g Ag)[/tex]
Explanation:
According to Avogadro's law, 1 mole of every substance contains avogadro's number [tex](6.023\times 10^{23})[/tex] of particles.
To calculate the moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given atoms}}{\text {Avogadro's number}}[/tex]
For Ag
given atoms = [tex]2.68\times 10^{11}[/tex]
avogadro's number = [tex]6.023\times 10^{23}[/tex]
Putting values in above equation, we get:
[tex]\text{Moles of}Ag=\frac{2.68\times 10^{11}}{6.023\times 10^{23}}[/tex]
1 mole of Ag weighs = 107.88 grams
Thus [tex]\frac{2.68\times 10^{11}}{6.023\times 10^{23}}[/tex] moles of Ag will weigh=[tex]\frac{107.88}{1}\times \frac{2.68\times 10^{11}}{6.023\times 10^{23}}=43.2\times 10^{-12}[/tex] grams.
