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5.6 Vapor pressure diagrams
Key points 1. Raoult’s law is used to calculate the total vapor
pressure of a binary system 2. The composition of the vapor in equilibrium
with a binary mixture is calculated by using Dalton’s law
3. The compositions of the vapor and the liquid phase in equilibrium are located at each end of a tie line
4. The lever rule is used to deduce the relative abundances of each phase in equilibrium
• The partial pressures of the components of an ideal solution of two volatile liquids are related to the composition of the liquid mixture by Raoult’s law
• The total vapor pressure (at some fixed T) changes linearly with the composition from pB* to pA* as xA changes from 0 to 1
5.6 Vapor pressure diagrams
pA = xApA∗ pB = xBpB
∗
p = pA + pB = xApA∗ + xBpB
∗ = pB∗ + (pA
∗ − pB∗ )xA
(a) The composition of the vapor • The vapor should be richer in the more volatile component than
the liquid • From Dalton’s law that the mole fractions in the gas, yA and yB are
5.6 Vapor pressure diagrams
yA =xApA
∗
pB∗ + pA
∗ − pB∗( ) xA
yA =pAp
yB =pBp
yB =1− yA
p = pA∗ pB
∗
pA∗ + pB
∗ − pA∗( ) yA
(a) The composition of the vapor
5.6 Vapor pressure diagrams
p = pA∗ pB
∗
pA∗ + pB
∗ − pA∗( ) yA
yA =xApA
∗
pB∗ + pA
∗ − pB∗( ) xA
(b) The interpretation of the diagrams
5.6 Vapor pressure diagrams
• The point a : the vapor pressure of a mixture of composition, xA
• The point b : the composition of the vapor that is in equilibrium with the liquid at that pressure
• Let’s interpret the horizontal axis as showing the overall composition, zA
• All the points down to the solid diagonal line is under such high pressure that it contains only liquid
• All points below the lower curve correspond to a system that is under such low pressure that it contains only a vapor phase
• Points that lie between two lines correspond to where two phases exist
(b) The interpretation of the diagrams
5.6 Vapor pressure diagrams
• Consider the effect of lowering p on a liquid mixture of overall composition a
• The vertical line with the fixed composition is “isopleth”
• At a1 : the liquid can exist in equilibrium with its vapor. The composition of the vapor phase is given by point a1’.
• Tie line : the line that join a1 and a1’ • At p1: there is virtually no vapor present;
however the tiny amount of vapor that is present has the composition a1’
• At p2: the overall composition is a2’’. The composition of liquid and vapor phases are a2 and a2’, respectively
• At p3: there is virtually no liquid • At a4: only vapor is present
(c) The lever rule
5.6 Vapor pressure diagrams
• To find the relative amounts of two phases α and β that are in equilibrium, we measure the distance lα and lβ along the horizontal tie line and use the lever rule
nαlα = nβlβ
5.7 Temperature-composition diagrams
Key points 1. A phase diagram can be used to discuss the
process of fractional distillation 2. Depending on the relative strengths of the
intermolecular forces, high- or low-boiling azeotropes may be formed
3. The vapor pressure of a system composed of immiscible liquids is the sum of the vapor pressure of the pure liquids
4. A phase diagram may be used to discuss the distillation of partially miscible liquids
(a) The distillation of mixtures
5.7 Temperature-composition diagrams
• The liquid phase lies in the lower part of the diagram
• Consider what happens when a liquid of composition a1 is heated
• The liquid boils at T2 ; the liquid has composition a2 and the vapor has composition a2’
• Simple distillation : The vapor is withdrawn and condensed
• Fractional distillation : the boiling and condensation cycle is repeated successively.
• The cycle can be repeated until in due course almost pure A is obtained in the vapor and pure B remains in the liquid ; theoretical plates
(b) Azeotropes
5.7 Temperature-composition diagrams
• A maximum in the phase diagram may occur when the favorable interactions between A and B molecules reduce the vapor pressure of the mixture
• Consider a liquid of composition a on the right of the maximum
• The vapor (at a2’) of the boiling mixture is richer in A. If the vapor is removed, the remaining liquid will move to a composition that is richer in B, a3
• As evaporation proceeds, the composition of the remaining liquid shifts towards B as A is drawn off
• The liquid reached the composition b • Azeotrope : the mixture for which the evaporation occurs without change of composition ; the distillation cannot separate the two liquids
(b) Azeotropes
5.7 Temperature-composition diagrams
• A minimum in the phase diagram may occur when the unfavorable interactions between A and B molecules increase the vapor pressure of the mixture
• Consider a liquid of composition a on the right of the minimum
• The mixture boils at a2 to give a vapor composition a2’.
• This vapor condenses to a liquid of a3 with the same composition.
• That liquid reaches equilibrium with its vapor at a3’
• The fractionation shifts the vapor towards b, but not beyond
(c) Immiscible liquids
5.7 Temperature-composition diagrams
• Distillation of two immiscible liquids • At equilibrium, there is a tiny amount
of A dissolved in B and a tiny amount of B dissolved in A
• p ≈ pA* + pB* • At temperature where p is equal to the
atmospheric pressure, dissolved substances are purged from their solution.
• The presence of the saturated solutions means that the ‘mixture’ boils at a lower T than either componet would alone because boiling begins when the total vapor pressure reaches 1atm, not when either vapor pressure reaches 1 atm.
• Steam distillation