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Consider the following data concerning an acetic acid/benzene mixture at 50 a C. The vapor pressure...

Consider the following data concerning an acetic acid/benzene mixture at 50 a C. The vapor pressure of pure benzene is 35.62 kPa at this temperature while pure acetic acid has a vapor pressure of 7.34 kPa. A 0.2973 mole fraction acetic acid solution is in equilibrium with a vapor that has a partial pressure of 28.16 kPa for benzene and 3.31 kPa for acetic acid.

What are the Raoult's law activity coefficients for solute and solvent in this system?

Is the heat of mixing in this system most likely zero, positive , or negative? Explain

If the partial pressure of solute is 0.484 kPa for a 0.0160 mole fraction acetic acid solution, what value for the Henry's law constant on the mole fraction scale would you predict for this solute in this solvent? You can assuming that the concentration of acetic acid is low enough that you are in the limiting law region.

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Amanda K answered 1 year ago
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