$$PV = nRT$$
where:
* P is the pressure in atmospheres (atm)
* V is the volume in liters (L)
* n is the number of moles of gas
* R is the ideal gas constant (0.08206 L atm / mol K)
* T is the temperature in Kelvin (K)
First, we need to calculate the number of moles of C2H2F4 vapor:
$$n = \frac{m}{M}$$
where:
* m is the mass of the gas in grams (g)
* M is the molar mass of the gas in grams per mole (g/mol)
The molar mass of C2H2F4 is:
$$M = 2(12.01 \ g/mol) + 2(1.01 \ g/mol) + 4(19.00 \ g/mol) = 64.06 \ g/mol$$
So, the number of moles of C2H2F4 vapor is:
$$n = \frac{0.100 \ g}{64.06 \ g/mol} = 0.001561 \ mol$$
Now, we can substitute the values of P, n, R, and T into the ideal gas law to calculate the volume:
$$V = \frac{nRT}{P}$$
$$V = \frac{(0.001561 \ mol)(0.08206 \ L atm / mol K)(295.45 \ K)}{0.0928 \ atm}$$
$$V = 0.404 \ L$$
Therefore, the volume of 0.100 g of C2H2F4 vapor at 0.0928 atm and 22.3°C is 0.404 L.
