How many atoms of carbon (C,12.01 g/mol) are in a diamond with a mass of 0.568 g?
1 answer:
2.85 × 10^22. A diamond with a mass of 0.568 g contains
2.85 × 10^22 atoms C.
Diamond is a form of pure carbon.
a) Convert <em>grams of C to moles of C</em>
Moles of C = 0.568 g C × (1 mol C/12.01 g C) = 0.047 29 mol C
b) Convert <em>moles of C to atoms of C
</em>
Atoms of C = 0.047 29 mol C × (6.022 × 10^23 atoms C)/(1 mol C)
= 2.85 × 10^22 atoms C
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