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 10^{5} N/m^{2} = 1.013 X
10^{5} Pa

1 gallon = 3.785 L

Answer #1

known terms

Chloroform (x_{1})=1500ppmv=0.15mol%

molecular weight of chloroform=119.35g/mol

vapour pressure of first component(chloroform)
p_{1}^{sat}=151mmHg

molecular weight of toulene=92.13g/mol

vapour pressure of first component(toulene)
p_{2}^{sat}=28.1mmHg

total pressure P=P_{1}^{sat} *
x_{1}+P_{2}^{sat} * x_{2} (where
x_{2}=1-x_{1})

=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%

A 10 mL of 120 mg/L solution of Styrene in water is injected
into a 125 mL vial at 20°C.
What will be the gas phase concentration at
equilibrium?
The Henry's Constant for Styrene is KH= 2.60
atm•L/mol
The molar mass of Styrene is 104 g/mol
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
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