Shortly after my post I realized that the atomic mass was the piece that I was missing, so to find n I did n=(mass)/(molecular mass), n=1gram/16, and after plugging that all in, I got a final density of 1.40 (which is basically much that of oxygen). Was I right to use n=1/16 or was it n=2...
Ok, I know I have to use the ideal gas law, but am not exactly sure how to apply that to finding the density.
PV=nRT (ideal gas law)
1atm (volume) = n(number of moles - can I just use 1 for ease?)(8.315 J(mol•K) (temperature)
Not quite sure where to go from here, any help would be...
I'm confused on this matter, and can't seem to find a clear explanation online or in my book. 3.00m^3 of gas at stp is at 0 degrees C, but does that mean the pressure is 1atm? Thanks for any help.