Question

The vapor pressure of pure component A is 42.0 kPa at 298 K. The
vapor pressure of pure component B is 29.0 kPa at the same
temperature. Which of the two substances has the lower normal
boiling point. Assuming an ideal liquid solution of A and B has
mole fraction A equal to 0.400, What are the partial pressures and
the total pressure over the liquid assuming Raoult’s law applies.
What is the composition of the vapor based on Dalton’s
law?

Answer #1

The vapor pressures of pure acetone and methanol are 165 kPa and
73.5 kPa, respectively, at 57.2oC. However, it was found that at
equilibrium at 57.2oC and 1 atm that xA=0.400 and yA=0.516, which
are the liquid and vapor phase mole fractions of acetone,
respectively. Using Raoult’s Law, calculate the activities and
activity coefficients of each component.

By measuring the equilibrium between liquid and vapor phases of
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Raoult’s law basis. The vapor pressures of the pure components at
this temperature are: pA* = 105 kPa and pM* = 73.5 kPa. (xA ia the
mole fraction in the liquid and yA...

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(XA). Use Raoult’s law to determine the vapor pressure
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vapor pressure. Show all equations and conversion factors

The vapor pressure of pure Freon 11 and pure Freon 12 at 25ᵒ C
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A single-stage liquid/vapor separation for the unknown molecule
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P2sat
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(b) Using your answer...

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