Question


A gaseous compound containing carbon and hydrogen was analyzed and found to cons
ist of between
80 and 90 percent carbon by mass. At 145ºC and 1.00 atm, the density of this compound is 2.45 g/L.
What is the molar mass of the compound?
Using Ideal Gas Law
PV = nRT = (mass/f.wt)RT
Solve for f.wt.
f.wt = (mass)RT/PV
= (2.45g)(0.08206L-Atm/mol-K)(418K)/(1-Atm)(1-L)
= 84.04 g/mole

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