Here's the problem:
A stream containing equimolar quantities of benzene, toluene, and ortho-xylene is fed into a flash separator.
a. If the flash separator operates at 50 ˚C, what are the minimum and maximum pressures (in kPa) where there is a two-phase region (liquid and vapor)?
(A: Max P =20 kPa, Min = 7 kPa)
So here's the approach I took:
If our species are equimolar in the feed, then assuming we have say, a 100 mol/s feed, we'd have mole fractions of each species =0.333
Now, I found the partial pressures of each species using the Antoine equation and the given A,B, and C values from my textbook:
Benzene: A=6.89272 B=1203.531 C=219.888 ==> p*=271.328 mmHg
Toluene: A=6.95805 B=1346.773 C=219.693 ==>p*=92.1128 mmHg
o-Xylene: A=7.00154 B=1476.393 C=213.872 ==>p*=25.4935 mmHg
Now with my understanding of the question, we're supposed to find the range of pressure values for which the entire system will be in the two phase region as opposed to just when the species themselves will enter the two phase region.
So with that understanding, I went to find the bubble pressure of the system:
P(bubble)=0.333271.238+0.33392.1128+0.333*25.4935 ==>P(bubble)=129.602 mmHg
And since my professor asked for it in kPa:
129.602(101.3kPa/760mmHg)=17.27kPa, which is substantially lower than the 20kPa in the given answer above.
Any ideas what I'm doing wrong here?