A 0.6-m3 rigid tank contains 0.6 kg of N2 and 0.4 kg of O2 at 300 K. Determine the partial pressure of each gas and the total pressure of the mixture. The gas constant for N2 is 0.2968 kPa·m3/kg·K and the gas constant for O2 is 0.2598 kPa·m3/kg·K.

Pnitrogen=3.18 kPa, Poxygen=1.62 kPa, Ptotal = 4.80 kPa

Explanation:

partial pressure equation becomes Ptotal = Pnitrogen + Poxygen

Partial pressure of Nitrogen

Pnitrogen = nRT/V

n=no of moles = mass/molar mass

mass of nitrogen=0.6kg

Molar mass of nitrogen gas=28gmol^-1

n=0.6/28=0.0214moles

R=0.2968 kPa·m3/kg·K

T=300k

V=0.6m^3

Pnitrogen = (0.0214 * 0.2968 * 300) / 0.6

Pnitrogen=3.18 kPa

Likewise

Poxygen=nRT/V

n=0.4/32=0.0125moles

R=0.2598 kPa·m3/kg·K

T=300k

V=0.6m^3

Poxygen = (0.0125 * 0.2598 * 300) / 0.6

Poxygen=1.62 kPa

Ptotal = 3.18+1.62 = 4.80 kPa