# Question e951f

${10}^{6}$ fluorine molecules have a mass of $\left({10}^{6} \cancel{\text{molecules"))/(6.022xx10^23*cancel("molecules}} \cdot \cancel{m o {l}^{-} 1}\right) \times 38 \cdot g \cdot \cancel{m o {l}^{-} 1}$ $=$ ??g#
Of course fluorine exists as the gaseous ${F}_{2}$ molecule at normal temperatures and pressures. A million fluorine molecules will not have a very large mass.
I used Avogadro's number in the calculation above, because I know that Avogadro's number (i.e. a MOLE) of fluorine ATOMS (i.e. $6.022 \times {10}^{23}$ fluorine atoms) has a mass of $19.00$ $g$ precisely. What is the mass of Avogadro's number of fluorine molecules?