Question

At 100C, the vapor pressures of hexane and octane are 1836 and 354 torr, respectively. A certain liquid mixture of these two components has a vapor pressure of 667 torr at 100C. Obtain the molar fractions in the liquid mixture and in the vapor phase. Suppose an ideal mixture.

Answer #1

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A solution contains 49.0 g of heptane (C7H16)and 59.0 g of
octane (C8H18) at 25 ∘C. The vapor pressures of pure heptane and
pure octane at 25 ∘C are 45.8 torr and 10.9 torr, respectively.
Assuming ideal behavior, calculate each of the following. (Note
that the mole fraction of an individual gas component in an ideal
gas mixture can be expressed in terms of the component's partial
pressure.)
A) The vapor pressure of heptane in the mixture
B) The Vapor...

The vapor pressures of benzene (C6H6) and hexane (C6H14) at 75°C
are 648 mm Hg and 921 mm Hg, respectively.
(a) If 330.0 g benzene is mixed with 730.0 g hexane at 75°C,
what are the mole fractions of benzene and hexane in this solution?
mole fraction of benzene mole fraction of hexane ?
(b) Assuming this is an ideal system that obeys Raoult's law,
find the partial vapor pressure of each component over the
solution. vapor pressure of benzene...

The vapor pressures of benzene and methylbenzene at 20°C are 75
Torr and 21 Torr, respectively. What is the composition of the
vapor in equilibrium with a mixture in which the mole fraction of
benzene is 0.75?

A solution contains 50.0 g of heptane (C7H16) and 50.0g of
octane (C8H20) at 25oC. The vapor pressures of pure heptane and
pure octane at this temperature are 45.8 and 10.9 Torr,
respectively.
Assuming ideal behavior, calculate the:
1) vapor pressure of each of the solution components in the
mixture
2) total pressure above the solution
3) composition of the vapor in mass percent
Please explain! Thank you.

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.

1. The following are the vapor pressures of some relatively
common chemicals measured at 20 °C:
Benzene, C6H6
80 torr
Acetic acid,
HC2H3O2
11.7 torr
Acetone, C3H6O
184.8 torr
Water, H2O
17.5 torr
Diethyl ether,
C4H10O
442.2 torr
Arrange these substances in order of increasing boiling point.
2. At 0.00 °C, hexane, C6H14, has a vapor
pressure of 45.37 mm Hg. Its ΔHvap is 30.1 kJ
mol-1. What is the vapor pressure of hexane at 12.9
°C?
The vapor pressure...

A solution of benzene (C6H6) and toluene (C7H8) is 27.0 %
benzene by mass. The vapor pressures of pure benzene and pure
toluene at 25 ∘C are 94.2 torr and 28.4 torr, respectively.
Assuming ideal behavior, calculate the following.
Calculate A) The vapor pressure of each of the solution
components in the mixture. B) The composition of the vapor in mass
percent.

If 12 mg of ethanol are dissolved in 25 mL of water
a. what are the mol fractions of the two liquids in the mix
b.the vapor pressures of pure ethanol and water at 25 C are
respectively 58.9 and 23.8 Torr. Calculate the vapor pressure of
the mix, assuming ideality
c. once the liquid has reached equilibrium with the vapor, what
will the mol fraction of the two liquids in the vapor phase be?

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...

7.1 Assume that the density of solid water is 920 kg m-3 and
that of liquid water is 1000 kg m-3. Calculate the change of the
melting temperature, T, of ice for the process of changing
pressure from 100 kPa to 1850 kPa. Use fusH = 6010 J mol-1 for
water.
7.2 At two temperatures, 85 K and 135 K, the vapor pressures of
a certain liquid were found to be 540 Torr and 830 Torr,
respectively. From this information,...

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