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Chemistry
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12 Dec 2019

An ideal solution at 298 K is made up of the volatile liquids A and B. As the pressure is reduced from 450 Torr, the first vapor is observed at a pressure of 70.0 Torr. Calculate xA.

PLEASE NOTE I've looked up the question. My professor DID NOT include pure vapor pressures of A and B in the question. That's why I'm posting this

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13 Dec 2019
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Related questions

An ideal solution at 298 K is made up of the volatile liquids A and B, for which the vapor pressures at that temperature (when pure) are PAº = 125 Torr and PBº = 46.3 Torr. As the pressure is reduced from 450 Torr the first vapor (first bubble) is observed at a pressure of 70.0 Torr. What is the mole fraction of A in the liquid mixture?


Volatile liquids A and B are completely miscible and form ideal solutions in all proportions. The pure vapor pressures at 298K are PA* = 500. torr and PB* = 200. torr. Using Excel may reduce the amount of time required to complete the following requested effort. Calculate, at 0.1 mole fraction intervals (xA = 0, 0.1, 0.2, . . . , 1) PA, PB, Ptotal, and yA, which is the vapor phase mole fraction of A. (i)Present these calculations in a suitable table. (ii)Plot PA, PB and Ptotal, vs. xA, and plot Ptotal, vs. yA on the same mole fraction scale as xA. All four plots should superimposed on the same axes as in the adjacent figure, but with labels for the lines/curves.

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