Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: hwgw on January 26, 2008, 08:25:42 PM
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Hi,
I have a question where I am given a sample of a mixture of gases (C2HF5 and C2H3F3) and was told to find the volume percentage of one gas.
Pressure = 0.449 atm
T= 288.15 K
Density= 1.79 g/L
I have also found the average molecular mass to be 94.266 amu.
So how can i approach this question to find the volume percentage of C2H3F3?
Do i use PV=nRT?
Thanks
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What's the molecular mass of C2HF5? What's the molecular mass of C2H3F3? What ratio of the two gasses gives an average molecular mass of 94.266?
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When asking for average molecular mass, is that (mass 1 + mass 2) / 2 ?
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No. You need to solve two equations:
x*M(C2HF5)+y*M(C2H3F3)=94.266 g/mol
x+y=1
x=percentage of C2HF5
y=percentage of C2H3F3
M=molar mass
94.266 g/mol = average molar mass of the mixture
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Thanks, that was really helpful. 8)
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You're welcome :)