Question

A 1 liter solution of diluted liquid chloroform with toluene is in a sealed container. The mole fraction of chloroform in the gas phase was measured at 1500 ppmv once the solution was prepared. The molecular weight is 119.35 g/mol for chloroform and 92.13 g/mol for toluene. The vapor pressure of chloroform and toluene are 151 mmHg and 28.1 mmHg, respectively.

What must the volume of liquid chloroform be in order to make a 1.0 liter total volume solution?

What is the total pressure in the gas phase?

Other Info:

R= 0.08206 atm•L/mole•K = 1.987 cal/mole•K = 8.314 J/mole•K

1 Joule = Newton • Meter

1 atm = 1.013 X 10⁵ N/m² = 1.013 X 10⁵ Pa

1 gallon = 3.785 L

Answer 1

known terms

Chloroform (x₁)=1500ppmv=0.15mol%

molecular weight of chloroform=119.35g/mol

vapour pressure of first component(chloroform) p₁^sat=151mmHg

molecular weight of toulene=92.13g/mol

vapour pressure of first component(toulene) p₂^sat=28.1mmHg

total pressure P=P₁^sat * x₁+P₂^sat * x₂ (where x₂=1-x₁)

=151*(0.15)+28.1(1-0.15)

=46.45mmHg

moles % of chloroform present in the solution y_A= (P_A^sat * x_A)/ P

=(151 * 0.15)/46.45

   =0.4876mol%