Question

A mixture of acetone (1) and chloroform (2) at 10 atmospheres creates an azeotrope at 64.6 ºC. At the azeotrope point, the mole fraction (x1) of acetone in the liquid phase is given as 0.335. The saturation vapor pressures of acetone and chloroform at 64.6 ° C are 1.31 and 0.98 atm, respectively. Calculate the activity coefficients of acetone and chloroform in azeotrope.

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.

Calculate the boiling temperature and the vapor phase mole
fraction y1 at 85 kPa of the binary mixture with the liquid phase
mole fraction x1 = 0.40. Consider the mixture ideal. The saturation
vapor pressures of the components in the mixture are given below
and are T (° C);
P1sat
= exp [14.3 - 2945 / (T + 224)]
P2sat
= exp [14.2 - 2943 / (T + 209)]

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...

Consider the benzene (1) + ethanol (2) system which exhibits an
azeotrope at 760 mmHg and 68.24°C containing 44.8 mole % ethanol.
At 68.24°C, the vapor pressures of pure benzene and ethanol are
519.7 mmHg and 503.5 mmHg respectively. Find the activity
coefficients of benzene and ethanol at the azeotrope and Calculate
the two parameters (A) for the Redlich / Kister
expansion.

The equilibrium vapour pressures of ethanol and chloroform at
45oC are 230.33 mbar and 578.0 mbar respectively. The Henry’s law
constants for ethanol at 45oC is 1030.3 mbar. A non‐ideal solution
of the two liquids has a mole fraction of ethanol in the liquid
phase of 0.115. The equilibrium vapour pressure of
chloroform above the solution is 533.7 mbar and the equilibrium
vapor pressure of the ethanol is 73.95 bar.
(a) Find the mole fraction of ethanol in the vapour phase...

1- Acetone (1) and Methanol (2) form
an azeotrope boiling at 55.7oC at 1 atm pressure, with a
composition x1 = 0.80. Calculate the van Laar
Coefficients for the system.
2- Perry (Table 13-1) quotes the following x,y,T data for
Acetone (1) and Methanol (2) at 101.3 kPa total pressure. Estimate
the van Laar constants A12 & A21.
T/oC
64.65
61.78
59.60
58.14
56.96
56.22
55.78
55.41
55.29
55.37
55.54
55.92
56.21
x1
0
0.091
0.190
0.288
0.401
0.501
0.579...

Given the equilibrium diagram P-x1y1 for
benzene (1)-toluene (2) mixture at 100 oC. Estimate the
approximate mole fraction of toluene of the vapor mixture for a 20
% benzene/80% toluene liquid mixture at bubble point. (5
points)

The binary system, acetone(1)-acetonitrile(2) conforms closely
to Raoult’s Law.
a) Using the vapor-pressure data, prepare a graph showing P vs.
x1 and P vs. y1 at 50ºC, and a graph showing T vs. x1 and T vs. y1
at 400 mm Hg. Thus when T is fixed, x1 and y1 vary with P, and when
P is fixed, x1 and y1 vary with T.
b) The mixture which has an acetone mole fraction of 0.405 is
heated slowly (so as...

A grey body is one whose absorptivity
1. does not vary with temperature and wavelength of the incident
ray
2. is equal to its emissivity
3. varies with temperature
4. varies with wavelength of the incident ray
A liquid is in equilibrium with its vapor at its boiling point.
On an average, the molecules in the liquid and gaseous phases have
equal
1. potential energy.
2. kinetic energy.
3.temperature. 4. intermolecular forces of attraction.
A liquid of density 1000 kg/m3...

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