A 5 gram sample of a gaseous substance occupies

Question

10 L at 48◦C and 697 torr. What is the
density of the gas under these conditions?
Answer in units of g/L

I first started converting the temperature to Kelvin, and the pressure to ATM. I then re-arranged the Ideal gas law to solve for the amount of mols under these conditons (.9171052 ATM*10 Liter)/(.0820157*321 Kelvin)=.3481 mols

I then solved for the molar mass by dividing the given mass and the amount of mols (14.36056 g/mol)

I'm stumped at the next step, and I was thinking I could directly divide the molar mass by the given volume in the question, but I don't think that's the correct way to do it?

Answer 1

you might be over thinking...

they give the mass and the volume

Answer 2

Does the pressure and temperature have any relation to the equation? I was thinking they might affect the density of the gas

Answer 3

for a given mass, the temperature and pressure affect the volume ... p v = n r t

but the volume is given here

Answer 4

Yeah, I just divided the mass and volume and got it right, I really did overthink it.
My bad!