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§8.4 adsorption at gas / solid interface
Levine:
pp. 397– 402 section 13.5 adsorption of gases on
solids
8.4.1 solid surface and specific surface area
Si
Suspending bond
Surface layer: enlarged interlayer space
Matter that is at or near an interface is not in the same state as those in the interior of
a phase. Owing to the suspending bond, solid surface is apt to react with other substances.
How de we stabilize the solid surface?
(1) Surface of solid: unbalanced force and suspending bond
8.4.1 solid surface and specific surface area
Single atom catalyst, is it real?
检索结果: 139(来自所有数据库)您的检索: 标题: (catalyst) AND 标题: (single atom) ...
(1) Surface of solid: unbalanced force and suspending bond
8.4.1 solid surface and specific surface area
arris Surface area Surface atom %
1 cm 6 cm2 3 10-8
1 m 6 104 cm2 30%
1 nm 6 107 cm2 ~ 100 %
(2) Degree of subdivision
(3) Specific area:
V
SSv = W
SSw =
The surface-to-volume / mass ratio
400 mJm-2 6 103 m2 = 2400 J
8.4.1 solid surface and specific surface area
Powder explosion in Baxian, Xinbei, Taiwan
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8.4.1 solid surface and specific surface area
Micropowder explosion: micropowder
is thermodynamically unstable.
(3) Danger of suspending powder
8.4.2 adsorption on solid surface
Solid can not lower surface energy by
shrinking its surface. How can solid lower
its surface energy?
gas
solid
Adsorbed
molecules
Adsorption of gas molecules
(1) The way to stabilize solid surface
8.4.2 adsorption on solid surface
Suspending bonds?
High surface energy?
Sorption: movement of a material from
one phase to another. Adsorption vs.
absorption
(2) Characteristics of adsorbents
8.4.2 adsorption on solid surface
Material
Specific
surface area
(m2 g−1)
MnFe2O4/activated carbon
magnetic composites
553
Activated Carbons from
Agricultural Residues
821
Activated carbon prepared from
lignin
931.53
Powdered activated carbon 1100---1230
Activated Carbon Fiber 1153.25
Commercial activated carbon 1200
Activated carbons from Iris
tectorum doped with ferric nitrate
1371
NaOH-activated carbon produced
from macadamia nut shells
1524
Adsorbate: the material being adsorbed.
Adsorbent: the material doing the
adsorbing.
chemical adsorption,
physical adsorption
chemisorption,
physisorption
(3) Kind of adsorption
8.4.2 adsorption on solid surface
Chemisorption
involves the formation of chemical bonds
between adsorbed molecule and solid surface,
and often involving the breaking of preexisting
bonds in the adsorbed molecule. In some cases
the chemisorption step requires an activation
energy.
physi-sorption
involves forces similar to the intermolecular
forces / weak interaction that lead to
condensation of vapors to liquid.
b.p.
(3) Kind of adsorption
8.4.2 adsorption on solid surface
Transition from physisorption to
chemisorption
The potential curve of adsorption
By following the transition from physical
absorption to chemical adsorption, catalysts
can activate reactant molecules at relatively
mild conditions. This is the basic principal
for heterogeneous catalysis.Physical adsorption
Transition state
Chemical adsorption
2Ni + H2
2Ni + 2H
−Ni−Ni−
H H −Ni−Ni−
H−H
(3) Kind of adsorption
8.4.2 adsorption on solid surface
sorption physisorption chemisorption
interaction
Thermal effect
temperature
Adsorbed layer
reversibility
selectivity
Comparison between chemical and physical adsorption
(3) Kind of adsorption
8.4.2 adsorption on solid surface
STHG −=
Adsorption is spontaneous, 0G
Entropy decreases during
adsorption 0S
0H
adsorption is a exothermic process
Therefore:
(4) Thermodynamic aspects of adsorption
Conditions for chemisorption
2W + N2 = 2 W-Nad
adsHm = D(N2) – 2X (W-N) < 0
2N
W-N2
DX
8.4.2 adsorption on solid surface
8.4.3 expressions of adsorption
The amount of adsorption (a) of a certain kind of solid
for certain gases is a function of T and p.( , )a a T p=
Ta ~ ~T p(1) For constant pressure: isobar (2) For constant adsorption : isochore
150 200 250 300 350 T/K
150
100
50
a/m
lg
-1
5.3
13.3
53.3 p
200 300 400T/K
20
p/k
Pa
13.3
53.3 a
40
60
80
8.4.3 expressions of adsorption
ads m
2
ln
a
Hp
T RT
= −
8.4.3 expressions of adsorption
(2) For constant adsorption : isochore
Clausius-Clappeyron equation.
Adsorption increases with increase of
pressure under low pressure. While at high
pressure, adsorption attains maximum value.
(3) adsorption isotherm:
20 40 60 80 p/atm
150
100
50
a/m
lg
-1
T-23.5
0
30
80
8.4.3 expressions of adsorption
Types of adsorption isotherm: Brunauer: five types of isotherms(3) adsorption isotherm:
8.4.3 expressions of adsorption
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(3) adsorption isotherm:
8.4.3 expressions of adsorption
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8.4.4 important adsorption isotherms
(1) Langmuir isotherm
1932 Noble Prize
USA,
1881/01/31 – 1957/08/16
for his discoveries and investigations
in surface chemistry.
Irving Langmuir
S: the total adsorption sites
S1: sites occupied by
adsorbed moleculesS
S1=
(1) Degree of coverage
(2) The basic assumptions
(1) The solid surface is uniform
(2) monolayer adsorption
(3) no intermolecular interaction
The uniform surface contains a fixed number
of adsorption sites. Each site holds only one
adsorbed molecule. The heat of adsorption is
the same for all sites and does not depends on
the fraction coverage .
8.4.4 important adsorption isotherms
1
2 1 1
k p bp
k k p bp = =
+ + 2
1
k
kb =
b (adsorption coefficient) :
the kinetic equilibrium constant of the adsorption and desorption
2krdes =
1(1 )adsr k p= −
(3) Adsorption and desorption rate and equilibrium
ads desr r=
Langmuir isotherm
(1) Langmuir isotherm
8.4.4 important adsorption isotherms
1
bp
bp =
+
at low pressure, bp > 1,
kam =
mV
V=
ap =
1
ap
ap =
+
1=
p
(1) Langmuir isotherm
8.4.4 important adsorption isotherms
For monolayer adsorption, the specific area can be thus estimated according to
W
LV
S
m
W
022400
=
1m
V bp
V bp=
+
1
m m
p p
V bV V= +
For Langmuir adsorption, when plotting
p/V against p, straight line can be obtained.
LRC=loading ratio correction
(1) Langmuir isotherm
8.4.4 important adsorption isotherms
Adsorption of hydrogen on different metal
surface.
Problems with Langmuir isotherm
Adsorption heat depends on the coverage, which suggests that the surface of adsorbent
is not uniform. Some sites are more active than the other.
Adsorption of nitrogen on graphitized carbon
black.
Condensation heat
(1) Langmuir isotherm
8.4.4 important adsorption isotherms
Condensation heat
Multilayer adsorption = condensation ?
Problems with Langmuir isotherm(1) Langmuir isotherm
8.4.4 important adsorption isotherms
BET isotherm: Brunauer-Emmett-Teller (1938) 1) Basic assumptions
(1) uniform surface;
(2) multilayer adsorption;
(3) the heat of the layer other than the first
layer is the condensation heat;
(4) desorption only occur at the layer
exposed to the gas
Multilayer adsorption = condensation ?Brunauer, S., Emmett, P. H. , Teller, E. Adsorption of gases in
multimolecular layers. J. Am. Chem. Soc. 1938, 60: 309-319
(2) adsorption BET isotherm
8.4.4 important adsorption isotherms
0
0
( ) 1 ( 1)m
V Cp
V pp p C
p
=
− + −
0
0
( )
1 ( 1)
mp p V CV
ppC
p
−=
+ −
0
0
1 1
( ) m m
p C p
p p V V C V C p
−= +
−
22400
mag
VLS =
0 0.2 0.4 0.6 0.8
p/p0
V/V
m
1
2
c = 1
c = 10
c = 100
c = 1000
III
III
BET absorption isotherm is valid for type I
through type III.
(2) adsorption BET isotherm
8.4.4 important adsorption isotherms
Measurement of specific area of solid with
BET
Fig. 1. Nitrogen-
adsorption
isotherms at -
195°C
Fig. 2. Linear B.E.T. plots of the
isotherms of Figure 1:
(2) adsorption BET isotherm
8.4.4 important adsorption isotherms
Metal catalyst: Pt, Pd, Ni, Fe
Oxide: Al2O3, SiO2Activated carbon: charcoal.
Catalysts or catalyst support
(2) adsorption BET isotherm
8.4.4 important adsorption isotherms
(2) adsorption BET isotherm
8.4.4 important adsorption isotherms
Both Langmuir and BET isotherms are
based on the assumption that the surface of the
solid is uniform and the adsorption heat is
independent of coverage.
(2) Freundlich isotherm
Freundilich adsorption isotherm can be
derived on the assumption that:
0
ads m ads m lnH H = −
1
na kp=1
ln ln lna k pn
= +
1ln ln lna k c
n= +
Valid for adsorption in
solution
(3) Freundlich isotherm
1
2 1 1
k p bp
k k p bp = =
+ + 2
1
k
kb =
ads0 exp
mHb ART
= −
8.4.4 important adsorption isotherms
Fig. 8. Comparison between experimental and computed
equilibrium data derived from the modified Freundlich
model in the case of adsorption of mixtures
(3) Freundlich isotherm
8.4.4 important adsorption isotherms
(3) Temkin adsorption isotherm
Temkin adsorption isotherm can be derived
on the assumption that:
0
ads m ads mΔ Δ (1 )H H = −
ln( )a k bp=
(4) Temkin isotherm
8.4.4 important adsorption isotherms
ln( )a k bp=
ln( )a k bc=
Other isotherms:
Frenkel–Halsey–Hill Adsorption Isotherm Model
Hygroscopic Growth Theory
Frumkin adsorption model
(4) Temkin isotherm
8.4.4 important adsorption isotherms
8.4.5 Theoretical consideration of heterogeneous catalysis
(1) Mechanism of heterogeneous catalysis
A surface reaction can usually be divided into five elementary steps:
diffusion
adsorption
reaction
desorption
diffusion
1) diffusion of reactants to surface;
2) adsorption of reactants at surface;
3) reaction on the surface;
4) desorption of product from surface;
5) diffusion of product from surface.
Which is r.d.s.?
8.4.5 Theoretical consideration of heterogeneous catalysis
Many surface reactions can be treated successfully on the basis of the following assumptions:
For unimolecular reaction over catalyst
Catalyzed isomerization or decomposition
A (g) +
A
B +
B
1) the r.d.s. is a reaction of adsorbed molecules;
2) the reaction rate per unit surface area is proportional to .
(1) Mechanism of heterogeneous catalysis
8.4.5 Theoretical consideration of heterogeneous catalysis
For bimolecular reaction over catalyst
Langmuir-Hinshelwood mechanism (L-H mechanism)
Langmuir-Rideal mechanism (L-R mechanism)
A (g)
B (g)
A B
Transition state
A-B
+
A (g) +
A-B +
A
+ B (g)
A B
(1) Mechanism of heterogeneous catalysis
8.4.5 Theoretical consideration of heterogeneous catalysis
Synthesis of ammonia
Langmuir-Hinshelwood mechanism (L-H mechanism)
Hydrogenation of ethylene
Langmuir-Rideal mechanism (L-R mechanism)
(1) Mechanism of heterogeneous catalysis
8.4.5 Theoretical consideration of heterogeneous catalysis
In middle 1970s, Ertl began to studied the
mechanism of Haber-Bosch process. Ertl used
LEED, AES, UPS, TDS to study this process and
measured the work function of N adsorption on
Fe(111), Fe(100) and Fe(110). He found the
dissociation of N2 on Fe surface, and the Haber-
Bosch process obeyed L-H mechanism.
He won 2017 Noble Prize.
(1) Mechanism of heterogeneous catalysis
8.4.5 Theoretical consideration of heterogeneous catalysis
For unimolecular reaction
Ar Akr =
According to Langmuir isotherm
1
bp
bp =
+ 1
A A
A A
kb pr
b p=
+
(2) kinetics for heterogeneous catalysis
Under low pressure, when bAPA > 1
kr =
1
A A
A A
kb pr
b p=
+
A Ar kb p=
pA
r
rmax
8.4.5 Theoretical consideration of heterogeneous catalysis
When bApA > 1
1
A A
B B
kb pr
b p=
+' A
B
pr k
p=
For example
Decomposition of ammonia over Pt3
2
[NH ]
[H ]r k=
1
A A
A
A A B B
b p
b p b p =
+ +
when competing adsorption
exists:
(3) Some phenomena for heterogeneous catalysis
8.4.5 Theoretical consideration of heterogeneous catalysis
The situation of the L-R mechanism is the same as that of unimolecular reaction over catalyst.
For L-H mechanism, small modification should be made.
A Br k =
A A B B
2
A A B B(1 )
kb p b pr
b p b p=
+ +
Rate~ partial pressure relation of L-H mechanism
pA
pB = constant
r
(3) Some phenomena for heterogeneous catalysis
8.4.5 Theoretical consideration of heterogeneous catalysis
Ununiformity of solid surface and catalysis
10-9 PH3, which is insufficient for formation
of monolayer, can destroy completely the
activity of Pt catalyst toward oxidation of
ammonia.
In 1926, Talyor proposed the active site model
(4) structure of catalyst--Active sites
1) Only the molecules adsorbed on the active
sites can lead to reaction.
2) The fraction of active sites on the catalyst
surface is very low.
8.4.5 Theoretical consideration of heterogeneous catalysis
Fe(100)Fe(111) Fe(211)
Fe(110)
Fe(210)
Active sites in iron catalyst
for ammonia synthesis
C7: active sites
The active site is in fact atom cluster
comprising of several metal atoms.
Increase of the degree of subdivision will
increase the ununiformity of catalyst surface
and increase the number of active sites.
(4) structure of catalyst--Active sites
8.4.5 Theoretical consideration of heterogeneous catalysis
The potential curve of adsorption Interaction between molecule and catalyst on
catalytic activity
(5) Activity of of catalyst
8.4.5 Theoretical consideration of heterogeneous catalysis
If bB is very large, even at low pB, A will be
very small. The reaction of A will be greatly
retarded. The impurities with high b is catalyst
poison.
(6) Poison and renewal of catalyst
1
A A
A A B B
kb pr
b p b p=
+ +
8.4.5 Theoretical consideration of heterogeneous catalysis