Asked by Anonymous
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?
Answers
Answered by
Olereb48
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
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
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.