The pressure and temperature of mixture of 4 kg of O2 and 6

The pressure and temperature of mixture of 4 kg of O2 and 6 kg of N2 are 4 bar and 27°C respectively. For the mixture determine the following : (i) The mole fraction of each component ; (ii) The average molecular weight ; (iii) The specific gas constant ; (iv) The volume and density ; (v) The partial pressures and partial volumes.

Solution

4 kg of O2 means 4/32 moles =.125

6 Kg of N2 means 6/28 moles= .2143

Total moles 0.3393

mole fraction of O2 = .37

Mole fracion of N2 = .63

Average MW: .37* 32 + .63*28 = 29.48

Specific Gas Constant R/ molar mass = 287/29.5 = 9.72

Volume and density of 4kg of O2 and 6Kg of N2 at 4 bar and 27 deg

use the perfect gas law PV =n1RT where n1 and n2 are calculated above, then add the individual component volumes