The Ideal Gas Law Demonstrates That.docx

The ideal gas law demonstrates that: PV=nRT in which n=m/M n= mole number m= mass or mass flow (kg/h) V= volume or volumetric flow (m3/hr) M= molecular weight of the gas for example Molecular weight of nitrogen (N2) =28 kg/kgmole In Normal conditions according to the latest SI definition P=100 kpa and T=0 C or 273.15 K R = gas constant =8.314 pa.m3/mol.K So, PV=(m/M)*R*T or

m(kg/h) = (P*V*M)/(R*T)

at Normal conditions then we have: m(kg/h) = M* 100* V (Nm3/h) / (8.314*273.15) or

m(kg/h) = 0.044 M* V (Nm3/h) example:

20 Nm3/h of Nitrogen is equal to: m = 0.044* 28 (molecular weight) * 20 (Nm3/h) m = 7 kg/h