Recent content by tomrh3

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...

It seems that it is indeed 1.

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.