A 1.00 carat pure diamond has a mass of 0.2 grams. How many carbon atoms are there within this diamond?

Oct 6, 2016

$\text{Number of carbon atoms} :$

$=$ $\frac{0.2 \cdot g}{12.01 \cdot g \cdot m o {l}^{-} 1} \times {N}_{A} {\text{ carbon atoms mol}}^{-} 1$

$=$ ??" carbon atoms"

Explanation:

${N}_{A}$ $=$ $\text{Avogadro's number}$ $=$ $6.022 \times {10}^{23} \cdot m o {l}^{-} 1$.

We know that in a $12.00 \cdot g$ mass of ""^12C atoms there are ${N}_{A}$ $\text{carbon atoms}$ precisely.