[customx]

I'm completely lost and have no idea how to approach this problem. It doesn't help that my teacher gave it as homework and there isn't even a similar problem in the book to compare it to

A compound has the empirical formula SF₄. At 20.0 Celsius, .100g of the gaseous compound occupies a volume of 22.1 mL and exerts a pressure of 1.02 atm. What is the molecular formula of the gas?

I've only written the following:
T = 293 K
Mass = .1 g
V = 22.1 mL
P = 1.02 atm
Molar mass of SF₄ = 108.65g

Can someone point me in the right direction please? thanks

[opti384]

A little hint is that you have to find out the molar mass of the compound in order to determine the molecular formula from the empirical formula

[MOTOBALL]

The next step is to remember that 1 mole of a gas occupies 22.4 L at STP (standard temp. & pressure).