There are [tex]2.55\times10^{23} [/tex] atoms in 1.7 mol Ca
Solution:
Initially we have to convert the given mass of calcium to moles of calcium, using its molar mass (referring to a periodic table, this is 40.08 g/mol
[tex]1.7 \text { g Ca }\left(\frac{1 \text{ mol Ca}}{40.08 \text{ g Ca}}\right)= 0.0424 \text{ mol Ca}[/tex]
Using Avogadro's number, [tex]6.022 \times 10^{23} \text{ particles per mol}[/tex] as [tex]1 \text{ mole }=6.022\times 10^{23}[/tex]
We can calculate the number of atoms present by [tex]0.0424 \text{ mol Ca}\times\frac{6.022 \times 10^{23}}{1 \text{ mol }}=2.55\times10^{23} \text { atoms Ca }[/tex]
