If we assume this two gases behave like ideal gas, then we use the ideal gas law [tex]PV=nRT[/tex], where P is the pressure, V is the volume, n number of moles, R gas constant and T the temperature in kelvins. As well as the density formula [tex]D=\frac{m}{V}[/tex]. First we calculate the molarity for Freon
[tex]CFCl_3 = (12+ 18.998 + 3 \times 35.453) =137.36\ g/mol[/tex].
The number of moles for freon are
[tex]D=\frac{m}{V} =\frac{ nM}{L} \implies n= \frac{DL}{M} = \frac{5.58 g \times L}{L \times 137.36g/mol}= 0.0406 mol[/tex]
We know [tex]n=\frac{m}{M}[/tex], so we insert this concept to our ideal gas equation
[tex]PV=n \times RT=\frac{m}{M} \times RT= \frac{mRT}{M}[/tex]. Since [tex]D=\frac{m}{V}[/tex], we insert this concept to the formula
[tex]PV=\frac{mRT}{M} \\P=\frac{mRT}{VM} = \frac{DRT}{M} \\\\\implies M= \frac{DRT}{P}[/tex]. The measurements take place in same conditions so,
[tex]M=\frac{DRT}{P} = \frac{4.38g}{L}\times \frac{1L}{0.0406mol} = 107.9\ g/mol[/tex]
