1. PRT 140 PHYSICAL CHEMISTRY PHASE DIAGRAMS
PN. ROZAINI ABDULLAH
PROGRAMME INDUSTRIAL CHEMICAL PROCESS

2. CHAPTER OUTLINE: Definition The phase rules Two component system
Vapour pressure diagrams
Temperature – composition diagrams
Liquid-liquid phase diagrams
Liquid – solid phase diagrams

3. Definition: Terms Definition Phase
A form of matter that is uniform throughout the chemical composition and physical state.
Number of phase denote by P.

4. Example 1 2
One phase
Donate by P= 1
Two phase
Donate by P= 2

5. 3
Three phase
Donate by P= 3 1 2
immiscible
Two phase
Donate by P= 2
Metal Metal 2
miscible
One phase
Donate by P= 1

6. Phase Transition & Phase Diagram:
Terms
Definition
Phase Transition
The spontaneous conversion of one phase into another phase, occurs at a characteristic temperature for a given pressure.
Transition Temperature
The temperature at which the two phases are in equilibrium and the Gibbs energy of the system is minimized at the prevailing pressure.
Phase Diagram
a pure substance shows the regions of pressure and temperature at which its various phases of thermodynamically stable.

8. Definition: Terms Definition Vapour pressure
The pressure of the vapour in equilibrium with the liquid
Sublimation vapour pressure
The vapour pressure of the solid phase
Boiling temperature
The temperature at which the vapour pressure of a liquid is equal to the external pressure
Normal boiling point, Tb
For the special case of an external pressure of 1 atm
Critical temperature, Tc
The temperature at which the surface disappears
Critical pressure, Pc
The vapour pressure at the critical temperature
Supercritical fluid
At the above the critical temperature
Melting temperature
The temperature at which under specified pressure the liquid and solid phases of a substance coexist in equilibrium

9. Normal freezing point, Tf
Definition:
Terms
Definition
Freezing temperature
Because a substance melts at exactly the same temperature as it freeze, the melting temperature of a substance is the same as freezing point.
Normal freezing point, Tf
The freezing temperature when the pressure is 1 atm
Triple point
A point at which the three phase boundaries meet.

10. Changes in Thermodynamic Properties
First Order
Second Order

11. Changes in Thermodynamic Properties
First Order
A transition for which the first derive of chemical potential with
respect to temperature is discontinuous.
Second Order
Which the first derivative of µ with the respect to the temperature
Is continuous but its second derivative is discontinuous.

12. Phase Rules: F = C – P + 2 Terms Definition Phase Rules
Which gives the number of parameters that can be varied independently (at least a small extent) while the number of phase in equilibrium is preserved.
F = C – P + 2
The phase rule
F : variance
C: components
P: number of phase at equilibrium

13. Phase Rules: F = C – P + 2 Terms Definition Variance, F
Is the number of intensive variables that can be change independently without disturbing the number of phase in equilibrium.
Components, C
Chemically independent constituent of a system.
The number of components in a system is the minimum number of type of independent species (ions or molecules) necessary to define the composition of all the phase present in the system.

14. Phase Rule For a one component system F = 3 – P
When only one phase is present, F = 2 and both p and T can be varied without changing the number of phases.
When two phases are present, F = 1 which implies that pressure is not freely variable if the pressure is set. This is why at a given temperature a liquid has a characteristic vapor pressure.
When three phases are present, F = 0. This special case occurs only at a definite temperature and pressure that is characteristic of the substance.

15. Phase Rule

16. Two Component Systems When two components are present in a system,
C = 2, so F = 4 – P.
If the temperature is constant, the remaining variance is F’ = 3 – P.
F’ indicates that one of the degrees of freedom has been discarded – in this case the temperature.
The two remaining degrees of freedom are the pressure and the composition

17. Two-components system
Vapour-pressure diagrams
The partial vapour pressures of the components of an ideal solution of two volatile liquids are related to the composition of the liquid mixture by Roult’s law:
: the vapour pressure of pure A
The total vapour pressure P of the mixture is therefore

18. Two Component Systems
This expression shows that the total vapor pressure (at a fixed temperature) changes linearly with the composition from pB* to pA* as xA changes from 0 to 1.

19. The variation of the total vapour pressure of binary mixture with the mole fraction of A in the liquid
when Roults’s law is obey

20. The Composition Of The Vapour
The composition of the liquid & vapour that are in mutual equilibrium are not necessarily the same.
The vapour should be richer in the more volatile component.
Dalton’s law: The mole fraction in the gas:
Provided the mixture is ideal:

21. The mole fraction of A in the vapour binary ideal solution express in terms of its mole fraction in the liquid
A is more volatile than B
In all cases, the vapour is richer than the liquid in A
Notes: if B is non volatile, so the = 0
At the temperature of interest, then it makes
No contribution to the vapour (yB = 0).

22. This equation can relate the total vapour pressure to the composition of the vapour

24. Two Component Systems
If we are interested in distillation, both vapor and liquid compositions are of equal interest.
So it makes sense to present data showing both the dependence of vapor and liquid composition upon mole fraction.

25. a : the vapour pressure of a mixture of composition, XA
b: the composition of the vapour that is in equilibrium with the liquid at the temperature.
Points that lie between the two lines correspond to a system in which there are two phases present, one a liquid and other a vapour.

26. Isopleth
Single liquid phase
a1’ is the vapour phase
Called as “tie line”
represent as phase in equilibrium
At this point, we may conclude that
at that pressure there is virtually no
vapour pressure. But, tiny amount of
pressure present at a1’.

27. Now consider the effect of lowering the pressure to P2: taking the system to a pressure and overall composition represented by point a2”.
This new P is below the vapour pressure of original liquid, so it vapourizes until the vapour pressure of the remaining liquid falls to P2.
The composition of such a liquid must be a2.
The composition of the vapour in equilibrium is given by the point a2’ at the other end of tie- line.

28. Pressure is further reduced to P3,
The compositions of liquid and vapour are represented by the points a3 and a3’.
a3‘ corresponds to a system in which the composition of the vapour is the same as the overall composition, we can conclude that the amount of liquid present is virtually 0, but the tiny amount of liquid present has composition a3.
A further decrease in P, take the system to point a4.
a4: only vapour present and its composition is the same as the initial overall composition of the system.

30. The Lever Rule
A point in the two-phase of a phase diagram indicates not only qualitatively that both liquid and vapor present, but represents quantitatively the relative amounts of each.
To find the relative amounts of two phases a and b that are in equilibrium, we measure the distances la and lb along the horizontal tie line, and then use the lever rule.

31. The lever rule:
nα : amount of phase α
nβ : amount of phase β

32. Temperature-composition diagrams
To discuss distillation we need a temperature- composition diagram instead of a pressure- composition diagram.
Such a diagram shows composition at different temperatures at a constant pressure (typically 1 atm).

33. The temperature-composition diagram corresponding to an ideal mixture with the component A more volatile than component B.
Successive boiling and condensations of a liquid originally of composition a1 is lead to condensate that is pure A.
The separation technique is called
fractional distillation.

34. Simple Distillation The vapor is withdrawn and condensed.
This technique is used to separate a volatile liquid from a non-volatile solute or solid.
Example:
Distillation of herbs for perfumery
and medicinal (herbal distillate)

35. Fractional Distillation
In a fractional distillation, the boiling and condensation cycle is repeated successively.
This technique is used to separate volatile liquids.

36. The efficiency of a fractionating column is expressed in terms of the number of theoretical plates, the number of effective vaporization and condensation steps that are required to achieve a condensate of given composition from a given distillate.

37. The number theoretical plates is the number of step needed to bring about a specified degree of separation of two components in a mixture.
The two systems shown correspond to (a) 3, (b) 5 theoretical plates.

38. Azeotropes
An azeotrope is a mixture of two (or more) miscible liquids that when boiled produce the same composition in the vapor phase as that is present in the original mixture.

39. Azeotropes
Although many liquids have temperature- composition phase diagrams resembling the ideal version, a number of important liquids deviate from ideality.
If a maximum occurs in the phase diagram, favorable interactions between A and B molecules stabilize the liquid.
If a maximum occurs in the phase diagram, unfavorable interactions between A and B molecules de-stabilize the liquid.

40. A high-boiling azeotrope .
When the liquid composition a is distilled, the composition of the remaining liquid changes towards
b but no further.

41. A low boiling azeotrope.
When a mixture at a is fractionally distilled, the vapour in equilibrium in the fractionating columns moves towards b and then remains unchanged.

42. Immiscible Liquids
Let’s consider the distillation of two immiscible liquids, such as octane and water.
The system can be considered as the joint distillation of the separated components.
Total vapor pressure p = pA* + pB*
Mixture boils when p = 1 atm, and so the mixture boils at a lower temperature than either component would alone.

43. The distillation of (a) two immiscible liquids can be regarded as (b) the join distillation of the separated components, and boiling occurs when the sum of the partial pressure equals the external pressure.

44. Liquid-liquid Phase Diagrams
Let’s consider temperature-composition diagrams for systems that consist of pairs of partially miscible liquids.
Partially miscible liquids are liquids that do not mix at all proportions at all temperatures.

45. Phase Separation
Suppose a small amount of liquids B is added to another liquid A at a temperature T’.
If it dissolves completely the binary mixture is a single phase.
As more B is added, A becomes saturated in B and no more B dissolves  2 phases.
Most abundant phase is A saturated with B.
Minor phase is B saturated with A.

46. The region below the curve corresponds to the composition and
The temperature–composition diagram for hexane and nitrobenzene at 1 atm.
The region below the curve corresponds to the composition and
temperature at which the liquids are
partially miscible.
The upper critical temperatures, Tuc, is the temperature above which the liquids are miscible in all proportions.
a’ – A saturated with B
a” – B saturated with A

47. Phase Separation
The relative abundance of each phase is given by the lever rule.
As the amount of B increases the composition of each phase stays the same, but the amount of each changes with the lever rule.
Eventually a point is reached when so much B is present that it can dissolve all the A, and system reverts to a single phase.

48. Example
A mixture of 50 g of hexane (0.59 mol C6H14) & 50 g of nitrobenzene (0.41 mol C6H5NO2) was prepared at 290K.
What are the compositions of the phases?
In what proportions /ratio do they occur?
To what temperature must the sample be heated in order to obtain a single phase?
Lets denote hexane by H and nitrobenzene by N

49. Answer Composition of the phases
The compositions of phases in eqm are given by the points where the tie line representing the tem intersects the phase boundary.
The point xN=0.41, T=290 K occurs in 2 phase region of the phase diagram
The horizontal line cuts the phase boundary at xN=0.35 and xN=0.83  composition of the 2 phases.
b) Proportions
Given by lever rule, the ratio of amounts of each phase = ratio of distances lα and lβ:
That is, there are about 7 times more hexane- rich phase than nitrobenzene-rich phase.
c) Temp needed to obtain single phase
- The temp at which the components are completely miscible is found by following isopleth upwards and noting the temp at which it enters the 1 phase region of the phase diagram = 292K

50. Critical Solution Temperatures
The upper critical solution temperature, Tuc is the highest temperature at which phase separation occurs.
Above the critical temperature the two components are fully miscible.
On the molecular level, this can be interpreted as the kinetic energy of each molecule over coming molecular interactions that want molecules of one type to come close together.

51. Critical Solution Temperatures
Some systems show a lower critical solution temperature, Tlc.
Below this temperature the two components mix in all proportions and above which they form two phases.
An example is water and triethylamine.

52. The temperature-composition diagram
For water and triethylamine.
This system shows a lower critical
temperature at 292 K.
The labels indicate the interpretation
of the boundaries.

53. Critical Solution Temperatures
The molecular reason for this is that water and triethylamine form a weak molecular complex. At higher temperatures the complexes break up and the two components are less miscible.
Some systems have upper and lower critical solution temperatures.

54. The temperature-composition diagram for the water and nicotine, which has both upper and lower critical temperatures.
Note the high temperatures for the liquid
(especially the water): the diagram corresponds to a sample under pressure.

55. Distillation Of Partially Miscible Liquids
What happens when you distill partially miscible liquids?
A pair of liquids that are partially miscible often form a low-boiling azeotrope.
Two possibilities can exist: one in which the liquid become fully miscible before they boil; the other in which boiling occurs before mixing is complete.

56. The mixture forms a low boiling azeotrope.
The temperature-composition diagram for a binary system in which the upper critical temperature is less then the boiling point at all composition.
The mixture forms a low boiling azeotrope.
Applies only to first drop.

57. The temperature-composition diagram for a binary system in which boiling occurs before the two liquids are fully miscible.

58. Liquid-solid Phase Diagrams
The knowledge of temperature-composition diagrams for solid mixtures guides the design of important industrial processes, such as the manufacture of liquid crystal displays and semiconductors.

59. The temperature–composition phase diagrams for two almost immiscible solids and their completely miscible liquids.
The isolepth through e corresponds to the eutetic composition, the mixture with lowest melting point.

60. Eutectics
The isopleth at e corresponds to the eutectic composition, the mixture with the lowest melting point.
A liquid with a eutectic composition freezes at a single temperature without depositing solid A or B.
A solid with the eutectic composition melts without any change of composition at the lowest temperature of any mixture.

61. Eutectics Solder – 67% tin and 33% lead by mass melts at 183 °C.
23% NaCl and 77% H2O by mass forms a eutectic mixture which melts at °C. Above this temperature the mixture melts.

62. Reacting Systems Many binary mixtures react produce compounds.
Gallium arsenide is a technologically important example – semiconductor.
Ga + As  GaAs

63. The constituent C is a true compounds, not just an equimolar mixture.
The phase diagram for a system in which A and B react to form a compound
C = AB.
The constituent C is a true compounds, not just an equimolar mixture.
If C melts and the liquid has the same composition, then we say it melts congruently.

64. Incongruent Melting

65. Exercises 1
At 90oC, the vapour pressure of methylbenzene is 53.3 kPa and that of 1,2-dimethylbenzene is kPa. What is the composition of a liquid mixture that boils at 90oC when the pressure is atm? What is the composition of the vapor produced?

66. Exercise 2
The vapour pressure of pure liquid A at 300 K is kPa and that of pure liquid B is 52.0 kPa. These two compounds form ideal liquid and gaseous mixtures. Consider the equilibrium composition of a mixture in which the mole fraction of A in the vapour is Calculate the total pressure of the vapour and the composition of the liquid mixture.

67. Exercise 3
Benzene and toluene form nearly ideal solutions. Consider an equimolar solution of benzene and toluene are 9.9 kPa and 2.9 kPa, respectively. The solution is boiled by reducing the external pressure below the vapour pressure. Calculate
The pressure when boiling begins
The composition of each component in the vapour
The vapour pressure when only a few drops of liquid remains.
Assume that the rate of vaporization is low enough for the temp to remain constant at 20oC.

68. Exercise 4
The following temperature/composition data were obtained for a mixture of two liquids A and B at atm, where x is the mole fraction in the liquid and y is the mole fraction in the vapour at equilibrium.
The boiling points are 124oC for A and 155oC for B. Plot the temperature/composition diagram for the mixture.
what is the composition of the vapour in equilibrium with the liquid composition (a) xA=0.50 and (b) xB=0.33?
θ/oC
125
130
135
140
145
150 xA
0.91
0.65
0.45
0.30
0.18
0.098 yA
0.99
0.77
0.61
0.25

69. Exercise 5
1-Butanol and chlorobenzene form a minimum-boiling azeotropic system. The mole fraction of 1-butanol in the liquid (x) and vapour (y) phases at 1.00 atm is given below for a variety of boiling temperatures.
Pure chlorobenzene boils at K
Construct the chlorobenzene-rich portion of the phase diagram from these data
Estimate the temp at which a solution whose mole fraction of 1- butanol is 0.3 begins to boil
State the compositions and relative proportions of the 2 phases present after a solution initially butanol is heated to K.
T/K
396.57
393.94
391.6
390.15
389.03
388.66
388.57 X
0.1065
0.1700
0.2646
0.3687
0.5017
0.6091
0.7171 y
0.2859
0.3691
0.4505
0.5138
0.5840
0.6409
0.7070