# How many carbon atoms in a 3.25*"carat" diamond?

Oct 16, 2016

$\text{Number of carbon atoms}$ $=$ $0.054 \cdot m o l \times 6.022 \times {10}^{23} \cdot m o {l}^{-} 1$ $=$ ??

#### Explanation:

$\text{1 carat}$ $=$ $\text{200 mg}$

$\text{Number of moles}$ $=$ $\text{Mass"/"Molar mass}$

$\text{Number of moles of carbon}$

$=$ $\frac{3.25 {\cancel{\text{ carat"xx200xx10^-3*cancelg*cancel"carat}}}^{-} 1}{12.011 \cdot \cancel{g} \cdot m o {l}^{-} 1}$

$=$ $0.054 \cdot m o l$, and we mulitply this by $\text{Avogadro's number}$ to get the number of carbon atoms.

$\text{Number of carbon atoms}$ $=$ $0.054 \cdot m o l \times 6.022 \times {10}^{23} \cdot m o {l}^{-} 1$ $=$ ??

And we go thru the same process for the aspirin sample:

$\frac{0.75 \cdot g}{180.16 \cdot g \cdot m o {l}^{-} 1} \times 6.022 \times {10}^{23} \cdot m o {l}^{-} 1$ $=$

$\text{How many aspirin molecules?}$