A 5 gram sample of a gaseous substance occupies

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?

you might be over thinking...

they give the mass and the volume

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

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

but the volume is given here

To calculate the density of a gas, you need to divide the mass of the gas by its volume. However, in this case, you have the molar mass and the number of moles but not the mass of the gas directly.

To find the mass of the gas, you can multiply the molar mass by the number of moles.

Mass of gas = Molar mass * Number of moles

Mass of gas = (14.36056 g/mol) * (.3481 mol) = 4.993 g

Now that you have the mass of the gas, you can calculate the density by dividing the mass by the volume.

Density = Mass of gas / Volume

Density = 4.993 g / 10 L = 0.4993 g/L

Therefore, the density of the gas under these conditions is 0.4993 g/L.

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

My bad!