Submit a question to our community and get an answer from real people.

Working with pV=nRT and I find for nitrogen gas, the n= about 28.01 amu and takes up a volume in dm^3 at a temperature K and a press in Pa.

if your trying to see the molar volume of one mol of nitrogen gas using the term 1 mol = n=28.01 g/mol taking a space of 22.710980(38) dm^3/ mol at 273.15 K at 100 kPA (1 bar). To use "n" in a balanced form, do you have to convert the temp and pressure to use = Nm^3 at 0 deg c at 1 bar.

Report as

I'm having trouble understanding your question. Why do you want to use the atomic mass number if you already have the number of moles?

Report as
it is true the amu will cancle out at the end of the equation so you can leave it out to start with. i was trying to be complet with the question.
another way to state my question is
is "n" in units of Nm^3 or not. if not then should i convert to that standard of Nm^3 and from what standard of temp and press is "n" at now.
Report as
n is the number of moles. I don't know what Nm^3 means...
PV=nRT is always in absolute temperature. Usually this is Kelvin, but Rankine works if you use the correct value for R.

One warning, I am only educated enough to use the ideal gas equation..
Report as