A solution is made using 15.7 percent by mass CH2CI2 in CHCI3. At 30 °C, the vapor pressure of pure CH2CI2 is 490 mm Hg, and the vapor pressure of pure CHCI3 is 260 mm Hg. The normal boiling point of CHCI3 is 61.7 °C. Using the mole fraction of CH2CI2 of 0.21, what is the vapor pressure of the solution in mmHg?

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Mole fraction of Ch2Cl2 in the solution is 0.2075.

 

D. (see pic)

E. What is the molality of CH2Cl2 in the solution?

F. What is the boiling point in degrees C of the solution? (Kb for CHCl3 is 3.67 C/m)

A solution is made using 15.7 percent by mass
CH2CI2 in CHCI3. At 30 °C, the vapor pressure of
pure CH2CI2 is 490 mm Hg, and the vapor
pressure of pure CHCI3 is 260 mm Hg. The normal
boiling point of CHCI3 is 61.7 °C.
Using the mole fraction of CH2CI2 of 0.21, what is
the vapor pressure of the solution in mmHg?
Transcribed Image Text:A solution is made using 15.7 percent by mass CH2CI2 in CHCI3. At 30 °C, the vapor pressure of pure CH2CI2 is 490 mm Hg, and the vapor pressure of pure CHCI3 is 260 mm Hg. The normal boiling point of CHCI3 is 61.7 °C. Using the mole fraction of CH2CI2 of 0.21, what is the vapor pressure of the solution in mmHg?
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