Excellent lecture. Just a stupid question, why can we write the ideal gas law pV=nRT as pv=RT for v = V/m? Does the molar mass is hidden in some constant?
The ideal gas law can be written in terms of mass as pV=mRT if u divide both sides by m you will have pv=RT where v=V/m. Here pay attention that R is the gas constant which different than R' the universal gas constant. When you write pV=nR'T, R' here is the universal gas constant since its used with the number if moles n The relation between the gas constant R and the universal gas constant R' is R=R'/M where M is the molar mass in kg/kmol. So originally pV=nR'T, if you replace R'=R*M in the equation you will have pV=mRT in the mass form.
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Excellent lecture. Just a stupid question, why can we write the ideal gas law pV=nRT as pv=RT for v = V/m? Does the molar mass is hidden in some constant?
The ideal gas law can be written in terms of mass as pV=mRT if u divide both sides by m you will have pv=RT where v=V/m. Here pay attention that R is the gas constant which different than R' the universal gas constant.
When you write pV=nR'T, R' here is the universal gas constant since its used with the number if moles n
The relation between the gas constant R and the universal gas constant R' is R=R'/M where M is the molar mass in kg/kmol.
So originally pV=nR'T, if you replace R'=R*M in the equation you will have pV=mRT in the mass form.