phase separations
DESCRIPTION
PHASE SEPARATIONS. Raoult’s Law. The partial vapour pressure of a component in a mixture is equal to the vapour pressure of the pure component at that temperature multiplied by its mole fraction in the mixture . Where P A =saturated vapour pressure of A - PowerPoint PPT PresentationTRANSCRIPT
PHASE SEPARATIONS
RAOULT’S LAW
The partial vapour pressure of a component in a mixture is equal to the vapour pressure of the pure component at that temperature multiplied by its mole fraction in the mixture.
Where PA =saturated vapour pressure of A =saturated vapour pressure of pure A =mole fraction of A in the solution
Raoult’s Law is obeyed by mixtures of similar compounds they are said to form IDEAL SOLUTIONS. The substances A and B form an ideal solution if the intermolecular forces A----A,A----B and B----B are all equal.
Examples of ideal mixtures are
1.
2.
3.
hexane and heptane
benzene and methylbenzene
propan-1-ol and propan-2-ol
VAPOUR PRESSURE / COMPOSITION DIAGRAMS FOR IDEAL MIXTURE LIQUIDS.
Ptotal=PA+PB
The partial vapour pressure of A at a particular temperature is proportional to its mole fraction. If you plot a graph of the partial vapour pressure of A against its mole fraction, you will get a straight line.
The mole fraction of B falls as A increases so the line will slope down rather than up. As the mole fraction of B falls, its vapour pressure will fall at the same rate.
BOILING POINT / COMPOSITION DIAGRAM FOR IDEAL MIXTURES
Notice again that the vapour is much richer in the more volatile component B than the original liquid mixture was.
The diagram just shows what happens if you boil a particular mixture of A and B. Notice that the vapour over the top of the boiling liquid has a composition which is much richer in B - the more volatile component.
Solutions of liquids which do not obey Raoult's Law are called non-ideal solutions.
There are two types of non ideal solutions 1.positive Deviation from Raoult's law 2. Negative Deviation From Raoult’s Law
Solutions which have a vapour pressure greater than that predicted from Raoult’s Law are said to show a positive deviation from the law.
E.g. Hexane and ethanol This is where the A--B interaction is
weaker than the A--A and the B--B interactions.
As a result the molecules escape from the mixture more easily than for an ideal solution.
VAPOUR PRESSURE COMPOSITION CURVE FOR NON IDEAL SOLUTIONS
1) POSITIVE DEVIATION
Maximum vapour pressure
This vapour pressure is greater than any other composition and either of the pure liquids
BOILING TEMPERATURE-COMPOSITION CURVES FOR NON IDEAL SOLUTIONS
1) POSITIVE DEVIATION
Minimum boiling point azeotrope
The same mixture will have a minimum boiling point lower than any other composition and either of the pure liquids
Solution with a vapour pressure lower than the calculated values are said to show a negative deviation.
E.g. Nitric acid and water This is where the A--B interaction is greater
than the A--A and the B--B interactions. It is more difficult for the molecules to
escape from the mixture than for an ideal mixture.
VAPOUR PRESSURE-COMPOSITION CURVE FOR NON IDEAL SOLUTIONS
2) NEGATIVE DEVIATION
Minimum vapour pressure
Which is less than any other composition and either of the pure liquids.
BOILING TEMPERATURE-COMPOSITION CURVE FOR NON IDEAL SOLUTIONS
2) NEGATIVE DEVIATION
Maximum boiling point azeotrope
This means there is a maximum boiling point which is higher than any other composition and either of the pure liquids
NOTE THE TERMS USED Minimum boiling point azeotrope
Maximum boiling point azeotrope
SIMPLE DISTILLATION Simple distillation is designed to evaporate a
volatile liquid from a solution of non-volatile substances; the vapour is then condensed in the water condenser and collected in the receiver.
FRACTIONAL DISTILLATION Fractional distillation is used to separate the
components of a mixture(miscible) of liquids by means of the difference in their boiling temperatures.
A mixture rich in the most volatile component distils over at the top of the column, where the thermometer registers its boiling temperature.
As distillation continues the temperature rises towards the boiling temperature of the next most volatile component.
The receiver is changed to collect the second component.
FUELS ARE OBTAINED FROM CRUDE OIL BY FRACTIONAL DISTILLATION
DISTILLATION AT REDUCED PRESSURE
High boiling liquids and many liquids which have a tendency to decompose near their boiling temperatures are often purified by distillation under reduced pressure, since lowering the pressure dramatically reduces the temperature at which a liquid will distil.
Distillation under reduced pressure always carries a slight risk of the apparatus *imploding.
*imploding -to collapse inwardly with force as a result of the external pressure being greater than the internal pressure, or cause something to collapse inwardly
VACUUM DISTILLATION Vacuum distillation is distillation at a reduced pressure.
Since the boiling point of a compound is lower at a lower external pressure, the compound will not have to be heated to as high a temperature in order for it to boil
Vacuum Distillation
Used to distill compounds that
have
High boiling point
undergoes decomposition on heating
at atm pressures
Or
STEAM DISTILLATION Steam distillation operates on the principle that
immiscible liquids exert their own vapour pressure so that when the mixture boils the sum of the vapour pressure equals one
Steam distillation is a method of distilling a compound at a temperature below its normal boiling point.
STEAM DISTILLATION
Ideal for separation of organic compound
s
Simple calculation Total vapour pressure=
P0A+P0
B
e.g. extraction
of eucalyptus
oil from eucalyptus (oils from plant materials)
Purification of phenylamine
and nitrobenzene
SOLVENT EXTRACTION Liquids that form two layers when mixed
provide an opportunity for purification of materials that prefer one layer more than the other.
For example, many organic chemicals are liquids that are very non-polar and separate from water because it is quite polar.
Partition-when the solute distributes itself between he two immiscible liquids.
Partition coefficient(k)-the concentration of the solute in each solvent at equilibrium is a constant ratio and the equilibrium constant for the system.
If cU and cL are the concentrations in the upper and lower layers then
cU/cL=k
k - Only applicable in dilute solutions and it varies with temperature
THE PARTITION COEFFICIENT WILL REMAIN CONSTANT UNDER THESE CONDITIONS:
1. the temperature is constant 2. the solvents are immiscible and do not react with each other 3. The solute does not react associate or dissociate in solvents.
SOLVENT EXTRACTION
Separated using a separating funnel
Partition coefficien
tSolute in
upper layer
Solute in
lower layer
Pdts of organic
preparations are often
dissolved in water
k - Only applicabl
e in dilute
solutions and it
varies with
temperature
SIMPLE QUESTION The mass of iodine used is 0.9656g and
25.0cm3 of the aqueous layer require 4.40cm3 of 0.01000 moldm-3 thiosulphate Ar(I)=127.
TOUGHER QUESTION The product of an organic synthesis, 5.00g of
X, is obtained in a solution in 1.00dm3 of water. Calculate the mass of X that can be extracted from the aqueous solution by
1. 50.0cm3 of ethoxyethane2. Two successive portions of 25.0cm3 of
ethoxyethane.The k of X between ethoxyethane and water is
40.0 at room temperature
INDUSTRIAL APPLICATIONS OF DISTILLATION
Petroleum
Rum
Fragrance
PETROLEUM
•BEER•VODKA
•RUM
Perfumes and Fragrances