Molar mass of CO=(12.01+16.00)g/mol=28.01g/mol
Molar mass of CO2=(12.01+16.00×2)g/mol=44.01g/mol
Assume that the mixture contains y% of CO and (1−y%) of CO2.
Average molar mass =[28.01×y%+44.01×(1−y%)] g/mol = (44.01 - 0.16y) g/mol
For the gaseous mixture :
Pressure, P = 740 mmHg
Density, d = 1.50 g/L
Molar mass, M = (44.01 - 0.16y) g/mol
Gas constant, R = 62.36 mmHg L / (mol K)
Temperature, T = (273 + 20) K = 293 K
PV=nRT
PV=(mM)RT
PM=(mV)RT
PM=dRT
M=dRTP
44.01−0.16y=1.50×62.36×293740
44.01 - 0.16y = 37.04
0.16y = 6.97
y = 43.6
100 - y = 56.4
The mixture contains 43.6% of CO and 56.4%ofCO2