Adsorption is the adhesion of molecules of gas, liquid, or dissolved solids to a surface. This process creates a film of the adsorbate (the molecules or atoms being accumulated) on the surface of the adsorbent. It differs from absorption, in which a fluid permeates or is dissolved by a liquid or solid.
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Content
• Adsorption
• Mechanism of Adsorption
• Types of Adsorption
• Factors affecting adsorption
• Adsorption Isotherm
• Adsorption of solute at the surface of
liquid
• Application of Adsorption
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The word coined by Henrich Kayser in 1881
• Adsorption is a surface phenomenon
• It is the deposition of molecular species onto the
surface
• Concentration of adsorbate on the surface of
adsorbent is high than that of bulk
Adsorbent : Surface on which adsorption occurs
Adsorbate : The molecular species that gets adsorbed on the surface
Adsorption is exothermic process in most of the cases
Adsorption
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Mechanism of
adsorption(WHY ADSORPTION OCCUR ? )
• It is a consequence of surface energy
• Molecules on the surface are not
wholly surrounded by other molecule
• These molecules experience some net
inward force of attraction which
cause surface tension
• In certain solids like transition metal,
the unutilized free valances at the
surface causes unbalanced inward
force
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a. POSITIVE ADSORPTION NEGATIVE ADSORPTION
o Van Der Waals force (weak)
o Enthalpy : 4-40 KJ/mol
o Multilayer formation
o Not specific
o Reversible in nature
o Occurs at low temperature
o Chemical Interaction (strong)
o Enthalpy : 40-400 KJ/mol
o Monolayer formation
o Specific in nature
o Irreversible in nature
o Occurs at high temperature
b. PHYSICAL ADSORPTION CHEMICAL ADSORPTION
Conc of adsorbate on surface < bulk
Ex : Dil. KCl is shaken with blood charcoal
Conc of adsorbate on surface > bulk
Ex : Conc. KCl is shaken with blood charcoal
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Factors affecting
adsorption
Temperature : TEMPERATURE ADSORPTION
GAS( adsorbate ) SOLID( adsorbent ) GAS ADSORBED HEAT
Pressure : With in pressure, adsorption to an extent till the saturation
level is achieved
Nature of the adsorbate : Easily liquefiable gas like NH3, HCl etc. are
adsorbed greater extent than permanent
gases like H2, O2, N2 etc.
Surface area of the adsorbent : SURFACE AREA ADSORPTION
EVAPORATION
CONDENSATION
(GAS BY SOLID)
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ADSORPTION ISOTHERM
At constant temperature, a plot between x/m (amount adsorbed by an adsorbent) is a
function of pressure or concentration
After Saturation -- No Adsorption
LIMITED SITES
ADSORBATE + ADSORBENT ADSORPTION
x/m
P Ps (SATURATION PRESSURE)
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FREUNDLICH ADSORPTION ISOTHERM
If
x/m = amount of gas adsorbed per gm of the
adsorbent
P = equilibrium pressure of adsorbate,
then over small range of P,
= K.P
n & k = Const.
o At low pressure : P
o At high pressure : P
X
m
1/n
m
x
x
m
PsPRESSURE (P)
x/m
m
x
= K.P
x
m = K.P
1/
n
=K.P
x
m
T= constant
EXTENTOFADSORPTION()
(FORM UNIFORM MOLECULAR LAYER)
0
A
B
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Plotting of FREUNDLICH ADSORPTION ISOTHERM
Limitation : Fails at high pressure
Plot Of log vs log P
x
m
log = log K + log P
x
m
1
n
INTERCEPT = log K
logx/m
log P
SLOPE = 1/n
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LANGMUIR ISOTHERM
ASSUMPTIONS
a. For monolayer only
b. Uniformity of sites(i.e. surface is
perfectly flat)
c. No interactions between
adsorbed moleculeA (gas) + M (surface) AM
Ka
Kd
Where,
Ka & Kd are rate const. for adsorption and desorption
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FORMULA
=
LIMITATION : VALID AT LOW PRESSURE AND MODERATELY HIGH TEMPERATURE
K =
Ka
Kd
Where,
=
NO OF ADSORPTION SITES OCCUPIED
NO OF ADSORPTION SITES AVAILABLE
At low pressure, K.P <<1,
At high pressure, K.P >>1,
= K.P
= 1
A
A
K.PA
1+K.PA
P =Partial pressure of AA
(atm
)
,
A
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FORMULA
V (1 - Z) { 1 - (1 - C ) Z }
V C.Z
=
mono
Z =
V = Volume of monolayer
coverage
C = a const
P
P *
Where,
mono
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TYPE OF ADSORPTION ISOTHERM
Type I Adsorption
• Monolayer
adsorption
• Langmuir
Adsorption Isotherm.
•Examples:
Adsorption of
Hydrogen (H) on
charcoal at
temperature near to
-180C
Type II Adsorption
•Deviation from
Langmuir model of
adsorption.
•Monolayer
formation.
•Examples :
Nitrogen (N2 (g))
adsorbed at -
195C on silica gel.
Type III Adsorption
• Deviation from
Langmuir model.
• Multilayer
formation
• Examples :
Adsorption
Isotherm are
Bromine (Br2) at
79C on silica gel
or Iodine (I2) at
79C on silica gel.
Type IV Adsorption
•At lower pressure,
graph is quite
similar to Type II.
•Monolayer
followed by
multilayer.
•Examples :
adsorption of
Benzene on silica
gel at 50C.
Type V Adsorption
•Similar to Type
IV.
•Type IV and V
shows
phenomenon of
capillary
condensation of
gas.
•Example :
adsorption of
Water (vapors) at
100C on
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Adsorption of solute from solution
o For multicomponent system
o Used to relate the change in concentration of component in contact with a
surface
with change in surface tension
o Due to presence of solute, Gives an exact relationship between adsorption and
change in surface tension of a solvent
o Gives an exact relationship between adsorption and change in surface tension
of
solvent due to presence of solute
(Gibbs adsorption equation)
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If
T = excessive concentration of solute for unit area of surface of
liquid
= surface tension
a = activity of solute
Then,
T =
For dilute solution,
T =
For surface active substances like soaps, detergents T is +ve
For surface inactive substances like most inorganic salts, sugar, T is -ve
a d
RT d a
c d
RT d c
2
2
2
2
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SEPERATION OF INNERT GAS ADSORPTION INDICATORGAS MASK
SILICA GEL : controlling humidity ACTIVATED CHARCOAL CHROMATOGRAPHY
20. CONCLUSION
o Adsorption is deposition of molecular species on the substance
o This process is seen in natural, biological, physical, chemical
system
o In industrial process like heterogeneous catalysis, in
pharmaceutical,
industry
o Thus adsorption plays a vital role in our day to day life requirements