A gas containing sulfur and fluorine analyzed as 29 % sulfur. A 140 g sample of a gas occupied a volume of 50.1 L with a pressure of 478.80 torr at 296.00 K. Enter the molecular formula of the compound.

I don't understand the question. Is the first statement and the second a continuation? That is, is the S containing compound the same as the 140 g of the gas?

Use PV = nRT to calculate n.
Then use n = grams/molar mass and calculate molar mass.

Use 29% S and 71% F to determine the empirical formula and use the molar mass to confirm. Post your work if you get stuck.

To determine the molecular formula of the compound, we need to use the given information. The first step is to calculate the number of moles of sulfur in the sample.

1. Calculate the mass of sulfur:
mass_sulfur = sample_mass * sulfur_percentage
mass_sulfur = 140 g * 0.29
mass_sulfur = 40.6 g

2. Convert mass of sulfur to moles:
moles_sulfur = mass_sulfur / molar_mass_sulfur
(you will need to look up the molar mass of sulfur, which is approximately 32.06 g/mol)
moles_sulfur = 40.6 g / 32.06 g/mol
moles_sulfur = 1.268 mol

3. Now that we know the moles of sulfur, we can determine the number of moles of the other element, fluorine, using the law of conservation of mass. Since there is only one sulfur atom in the compound, the number of moles of sulfur is equal to the number of moles of the compound. Therefore, we have 1.268 moles of the compound.

4. Calculate the mass of fluorine:
mass_fluorine = sample_mass - mass_sulfur
mass_fluorine = 140 g - 40.6 g
mass_fluorine = 99.4 g

5. Convert mass of fluorine to moles:
moles_fluorine = mass_fluorine / molar_mass_fluorine
(you will need to look up the molar mass of fluorine, which is approximately 18.998 g/mol)
moles_fluorine = 99.4 g / 18.998 g/mol
moles_fluorine = 5.225 mol

6. Finally, we can determine the ratio of moles of each element in the compound. Divide the moles of sulfur and fluorine by the smallest number of moles (in this case, sulfur):
moles_sulfur = 1.268 mol / 1.268 mol = 1
moles_fluorine = 5.225 mol / 1.268 mol ≈ 4.116

The simplest whole-number ratio between sulfur and fluorine is approximately 1:4. Therefore, the molecular formula of the compound is SF4 (Sulfur Tetrafluoride).