Question
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?
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?
Answers
Scott
you might be over thinking...
they give the mass and the volume
they give the mass and the volume
Jason
Does the pressure and temperature have any relation to the equation? I was thinking they might affect the density of the gas
Scott
for a given mass, the temperature and pressure affect the volume ... p v = n r t
but the volume is given here
but the volume is given here
Jason
Yeah, I just divided the mass and volume and got it right, I really did overthink it.
My bad!
My bad!