Phase Equilibrium Note
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Transcript of Phase Equilibrium Note
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PHASE EQUILIBRIUM
Miscible liquids- 2 liquids dissolves completely to produce homogenous solution
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IDEAL SOLUTION = obeyRaoults Law
NON-IDEAL SOLUTION do not obey Raoults LawNegative deviation Positive deviation
The intermolecular forcesof attraction between A A,B B and A B (aftermixing) are equal
The intermolecular forces ofattraction between A B isstronger than B B and A A
The intermolecular forcesattraction between A B isweaker than B B and A
No change in volume aftermix A & B
Decreases in volume after mixing Increases in volume aftermixing
No enthalpy change onmixing( heat is neitherliberated nor absorbed)
Temperature increases aftermixing-Heat is liberated (the heat energy
released to form new bonds isgreater than the heat energyabsorbed to break the bonds inpure liquids)
Temperature decreases aftermixing-Heat is absorbed (the heat
energy released to form newbonds is less than the heatenergy absorbed to break thebonds in pure liquids)
Obey Raoults law :The partial vapourpressure of a component (A)in a solution at a giventemperature is equal to thevapour pressure of pure liquid(A) at the same temperature,multiplied by the mole
fraction of the component(A) in the solution.Or PA = PA XA .(solution)PT = PA+PB //// XA + XB = 1XA = PA / PT (gas)
Actual vapour pressure is lowerthan the predicted by RaoultsLaw
Actual vapour pressure ishigher than the predicted byRaoults Law
Decreases the tendency ofmolecules to escape from theliquid mixture
Increases the tendency ofmolecules to escape from theliquid mixture
Minimum vapour pressure Maximum vapour pressure
Produce azeotropic solution solution where the composition of thvapour is the same as the composition of the solution at constantboiling pointAzeotropic mixtures withmaximum boiling point
Azeotropic mixtures withminimum boiling point
Example : most liquids withsame functional group-ethane butane-ethene butane-benzene-methylbenzene-Ethanol-buthanol-water - methanol
HCl H2OPropanone-CHCl3HNO3 H2O
Ethanol-water
Ethanol-benzene
Benzene-methanol
Vapour pressure-compositiondiagram
NOTE** A is high in v.p , lowb.p, thus more
volatile
Vapour pressure-compositiondiagram
Vapour pressure-compositiondiagram
n -compos n -compos on Boiling point-compositiondia ram
100% A100% B100%100% B100% B0% A
b.p
B
Vp PA
Vp PB
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DISTILLATION :
1. Simple distillation for separation of solutions with a big differences in b.p
2. Fractional distillation for separation of solutions with small differences in b.p
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Miscible ideal solution(example : mixture of benzene-methylbenzene)
1. Benzene is more volatile thanmethylbenzene.
2. If 0.2 moles of benzene (0.8methylbenzene) is heated,itwill boil at T1 and producedmixture of C1 which is richerin benzene .
3. As vapour C1 pass the coolercolumn, it condenses andform a liquid of compositionC1.
4. As the beads graduallyheated,its hot vapour allow torevapourised the C1composition liquid
5. Repeating of condensationand vapourising increases thepercentage of benzene invapour.
6. First distillate is benzene(lower bp),methylbenzene will bethe residue// it will bedistilled at 110C(bp).
Miscible non-ideal solution Negative deviation (example : water -nitric acid)
Miscible non-ideal solution Positive deviation
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3. Steam distillation - to separate liquids with high bp which might decompose on heating
-mainly for two immiscible liquids with one of the component iswater.
- Steam distillation is used to extract fragrant oils from plants (makingperfume) and purify
organic compound
-To carry out this process, the liquid must be immiscible with water,have a relatively high RMM and
high vapour pressure(100C)
Mixture of two Immiscible liquids.
Immiscible liquid liquids do not dissolve in one another Two of the immiscible liquids (A & B) are mixed, it form two separate layers Lower density liquid top layer Higher density liquid bottom layer The intermolecular forces of attraction between their molecules are different Example: benzene and water, mercury and water, chlorobenzene and water,
nitrobenzene and water Water is a polar molecule Benzene, chlorobenzene and nitrobenzene are non-polar molecule with van der Waals
forces of attraction and mercury atoms are bonded to each other with metallic bond. PT = PA + PB where PT = Total pressure of the liquid mixture,
PA = Vapour pressure of pure liquid A,P
B= Vapour pressure of pure liquid B
Method of distillation and purification: Steam distillation and followed by separationprocess using separation funnel
mA / mB = PAMA / PBMB mA andmB = mass//percentageby mass of A and B respectively
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MA and MB = rmm A and Brespectively.
Exercises.
1999 Paper 2
2004
Paper 1
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2007 paper 2
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Distribution of a Solute between two solvents
1. The partition law a solute will distribute itself between two immiscible solvents suchthat the ratio of the concentration of the solute in both solvents is equal to a constant, at afixed temperature.
Solvent A Concentration of X in solvent A [g/dm3 or mol/dm3] = K
Concentration of X in solvent B [g/dm3 ormol/ dm3]
Solvent BK is a partition coefficient ..constant at fixed temperature and has
no unit.
2. The partition law can only be used under this condition:a) Solution must be dilutedb) The solute must exist in the same molecular state in both solvents.
-the solute can not undergo dissociation or association (usually formation of dimer in case of carboxylic acid) in one of the solvents.-e.g distribution between butanoic acid between water and methylbenzene
Benzoic acid will partially dissociate in water : CH3CH2CH2COOH + H2OCH3CH2CH2COO-- + H3O+
Benzoic acid will associate in methylbenzene : 2 CH3CH2CH2COOH (CH3CH2CH2COOH)2
(formation of dimer)
Or Benzene
Water
c) The temperature is constant
Solvent Extraction :
Apply partition law.
Organic compound- in aqueous layer
Ether extraction ---used ether asextracting solvent.
Advantage of ether extraction :
Ether almost immiscible with water
Most Nk
n
X
X
HI
H+
+ I-
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CHROMATOGRAPHY
- technique used to separate the components of a mixture by distributing the mixture betweentwo immiscible phases..stationary phase and mobile phase.
- 2 types of chromatography
1. adsorption chromatography -