# How do you convert .4190 moles of oxygen difluoride to particles of oxygen difluoride?

Mar 17, 2017

#### Explanation:

You can go from moles of oxygen difluoride, ${\text{OF}}_{2}$, to molecules of oxygen difluoride by using Avogadro's constant.

Avogadro's constant is basically the definition of the mole. In this case, you know for a fact that in order to have $1$ mole of oxygen difluoride, you need to have $6.022 \cdot {10}^{23}$ molecules of oxygen difluoride in your sample.

Since your sample contains a little under $0.5 = \frac{1}{2}$ moles, you can expect to have a little under $\frac{1}{2} \cdot 6.022 \cdot {10}^{23}$ molecules.

More specifically, your sample will contain

0.4190 color(red)(cancel(color(black)("moles OF"_2))) * overbrace((6.022 * 10^(23)color(white)(.)"molecules OF"_2)/(1color(red)(cancel(color(black)("mole OF"_2)))))^(color(blue)("Avogadro's constant"))

$= \textcolor{\mathrm{da} r k g r e e n}{\underline{\textcolor{b l a c k}{2.523 \cdot {10}^{23} \textcolor{w h i t e}{.} {\text{molecules OF}}_{2}}}}$

The answer is rounded to four sig figs, the number of sig figs you have for the number of moles of oxygen difluoride.