Catalysis Introduction
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Transcript of Catalysis Introduction
ChE 511 - Catalysis Prof. Dr. Işık Önal
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CATALYSTSUsed in Chemical and Allied Industries. Approximately 1/3 of Material
GNP of U.S. involves a catalytic process somewhere between raw materials and finished products.
TYPES OF CATALYTIC PROCESSESHomogeneous : Catalyst is in a solution with at least one of the
reactants.Heterogeneous : Involves more than one phase where usually
catalyst is in solid phase and reactants and products are gases or liquids.
MOST IMPORTANT FUNCTIONS OF A CATALYSTActivity
SelectivityLong-term stability
ChE 511 - Catalysis Prof. Dr. Işık Önal
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ChemicalReactor
ChemicalKinetics
DesignMathematicsFluid FlowThermo.
Mass Transfer
Heat Transfer
Materials Process Control
Economics
ProductMarketing
ChemicalProcessDesign of a
chemicalreactor
Bench-scaleBatch Reactor
Bench-scaleContinuousReactor
Pilot Plant Demonstration Plant----Operating Plant
LECTURE-1
ChE311
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LECTURE-1
ChE311
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Category Typical PlantCapacity Price Waste Products
Tons/yr $/1b lb/lb___________________ _______
Petroleum Refining 106 - 108 0.1 0.1Commodity Chemicals 104 – 106 0.1-2 1 - 3Fine Chemicals 102 – 104 2 – 10 2 – 10Foods 1 – 50Materials 0 - Pharmaceuticals 10 - 103
Very different tasks in each category for a Ch.E.
ImportantIn petroleum + commodity Low-costFine chemicals Patent
protectionFoods & pharmaceuticals Patents, trademarks
Marketing, advertising
LECTURE-1
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DEFINE PROBLEM/OBJECTIVESActivitySelectivity ChemicalDeactivation DiffusionalRegeneration MechanicalCostAvailability
CATALYST RESEARCHCatalyst Prop. Catalytic Mech.Catalyst Rate EquationSupport Reaction StepsPromoters EnergeticsPreparation AdsorptionPretreatment Mass & Heat Pellet Form Transfer
PATTERNS OF BEHAVIORTHEORIES OF
CATALYSIS
CATALYTIC CHEMISTRY
Surface Chemistry and Physics Physical Chemistry Solid State Physics Patents Literature Experimental Programs
CHEMICAL ENGINEERING
Process Analysis Reaction Engineering
Economics
PROCESS ENGINEERING
Comparison with Similar Processes
PROCESS NEED
New Process Modification of Old
Process
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CATALYST DESIGN
New Experimental Commercial
CATALYST TESTINGExploratoryBench ReactorsModel Reactions
CATALYST PREPARATIONLaboratory MethodsSmall ScalePreparation Parameters
COLLOID CHEM.TechniquesDescription
COMMERCIAL MANUFACTUREScale-up of ProceduresPlant FormulationsLarge Batches
UNIT OPERATIONSPrecipitationWashingDryingCalcining Solid Handling
REACTOR ENG.Unit Design and OperationData AnalysisModeling
PILOT UNIT TESTINGReal FeedsProcess ConditionsProcess VariablesLife-time StudiesScale-up Data
PROCESS DESIGNProcess and Economic OptimizationPlant Design
CHEMICAL AND MECHANICAL ENG.Plant DesignMaterialsSpecifications
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TARGET REACTION
STOICHIOMETRIC ANALYSIS
THERMODYNAMIC ANALYSIS
MOLECULAR MECHANISM
SURFACE MECHANISM
REACTION PATH
CATALYST PROPERTIES
CATALYTIC MATERIALS
PROPOSED CATALYSTSteps in catalyst design
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TARGET REACTION
LIST STOICHIOMETRIC REACTIONS
GENERATE THERMODYNAMIC PARAMETERS
PROPOSE MOLECULAR MECHANISMS
PROPOSE SURFACE MECHANISMS
DEFINE CATALYST PROPERTIES
PROPOSED CATALYST
CHEMISTRYDATA BASE
THERMODYNAMICDATA BASE
REACTIONDATA FILE
SURFACE CHEMISTRY FILE
CATALYST PROPERTY FILE
OperatorInput
OperatorInput
OperatorInput
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Propylene Oxide Formation on Cu2O (001) Surface
(by utilizing, DFT, VASP code)
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11
Relative Energy Profile of Propylene Oxide, Propionaldehyde and Allyl Radical Formation
-4,5
-4
-3,5
-3
-2,5
-2
-1,5
-1
-0,5
0
0,5
1R
elat
ive
Ene
rgy
(eV
)
Surface Intermediate Type Mechanism and Acrolein Formation Pathway on Cu2O(001)
C3H6 (ads)
OMMP2(ads)
PO(ads)
PO (g)
Allyl-radical(ads)
Allyl-radical(g)
Acetone (ads)
Acetone (g)TS(Acetone)
TS(Acrolein) Acrolein (g)
Acrolein(ads)
TS (PO)
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R1
R2
R3A
B
C
CH2=CH2 + O2
Ag
Pt
PdCl2, CuCl2, HCl
Homogeneous
OCH2
CH2
2 CO2 + H2O
CH3CHO
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REACTION MECHANISM •KINETICS (MACROSCOPIC LEVEL)
•DYNAMICS (MICROSCOPIC LEVEL)
HETEROGENEOUS CATALYSIS BY
METALS
SYNTHESIS OF CATALYSTS CHARACTERIZATION OF CATALYSTSSOLID STATE CHEMISTRY
SURFACE AND COLLOID CHEMISTRY
ORGANOMETALLIC CHEMISTRY
STRUCTURE, TEXTURE, SPECTROSCOPY, AND DIFFRACTION
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HOMOGENEOUS CATALYSIS
CH3-CH=CH2 + CO + H2
CH3-CH2
CHO
CH3isobutylaldehyde
CH3-CH2-CH2-CHOn-butylaldehyde
CoComplexLiq. Phase Catalyst
Propylene
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HETEROGENEOUS CATALYSIS
+ H2C=CH2
Solid Phase Catalyst
Acid Catalyst
C2H5
Benzene Ethylene Ethylbenzene
C2H5
Ethylbenzene
Dehydrogenation
CatalystC2H5-CH=CH2
[Fe3O4-type] Styrene
(Phosphoric
Acid Type
or
ZSM-5 Type)
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C + H2O
Coal or biomass
CO+ H2
“Syn-gas”
CH4 + O2
Natural Gas
CH3OH
Methanol
+ COAcetic Acid
Cellulose Acetate
(base for photographic film)
+Cellulose
Ag HCHO Formaldehyde
Polymers
(fabrics and building materials)
(CH2)n
Petrol (fuel)
ZeoliteCH3
Toluene (solvent)
Zeolite
Cu/ZnO
CH4 Methane Substitute
Natural GasNi/Al2O3
(CH2)n
Polyethylene (polyethene)
Ru
Alkanes, Alcohols,
Alkenes (fuels, aviation or
diesel), solvents,
detergents
Fe, Co
CH2OH
CH2OH
And related glycols (antifreeze agents)
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Pote
ntia
l Ene
rgy
Reaction Coordinate
Reactants
Ehet
Ehom
ΔH
Products
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1 2 3 4 5 6 70
1
2
3
4
5
6Lo
g 10
(rat
e co
nsta
nt),
arbi
trar
y un
its
103/T
Ahet
Ahom
Homogeneous Reaction Heterogeneous
Reaction
Measurable Range
YX
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SURFACE ASSISTED (CATALYTIC) REACTIONS
Example: Catalytic Hydrogenation of EthyleneC2H4 + H2
ΔG C2H6
Postulated Mechanisms:For Homogeneous Reaction:
C2H4 + H2ΔG* C2H4 . H2 Activated Complex
Where ΔG* = Free Energy of Activation
C2H6
For Heterogeneous Reaction:
C2H4 + [S]1ΔG1 C2H4[S]1
H2 + C2H4[S]1ΔG2 C2H4[S]1 H2
C2H4[S]1 H2ΔG3 C2H6 + [S]1
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Published Data from Boudart:
CuO-MgO
Catalyst
At 600K;
A difficult homogeneous reaction is replaced by a more easily executed heterogeneous surface reaction involving adsorbed C2H4 .
(Eley-Rideal Mechanism)These are simply phenomenological models, not mechanisms. The actual mechanism is quite complex.
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HETEROGENEOUS CATALYSIS MUST ALWAYS BE PRECEDED BY ADSORPTION
desorptionAB
Cadsorption
A
B
C
Surface Reaction
Surface Migration
Two possible ways in which heterogeneous catalysis proceeds at a surface; the Langmuir-Hinshelwood Mechanism (left) and the Eley-Rideal Mechanism (right)
A
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C-C=C-C
HMethyl Cyclopropane
Butene ButaneC-C-C-C
Metal
Support
A bifunctional catalyst such as platinum on Al2O3 facilitates the isomerization of methylcyclopropane to 2-butene as well as the
hydrogenation of 2-butene to butane (after Boudart)
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Physical Adsorption•Weak Forces of Molecular Interaction (Van der Waals)
•Small Heats of Adsorption (10-40 kj/mol)
•Occurs only at ~Tb.p.
•Equilibrium rapidly attained, low E
•Highly reversible
•Multilayer coverage possible
•Nonspecific, almost indistinguishable from condensation
•In general, not responsible for catalysis; however may help to form chemisorption precursors
•Important for determination of total surface area and pore size of catalyst support
Chemisorption•Formation and Rupture of Chemical Bonds
•Large Heats of Adsorption (80-400 kj/mol)
•No such restriction at high T
•Nonactivated: Low E Activated: High
• Often Irreversible
•Less than a monolayer
•Highly specific (a function of a particular crystalline face)
•Necessary for catalysis
•Important for determination of active-center surface area and elucidation of surface reaction kinetics
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Oxidation of CO to CO2 Pd-Ce0.75Zr0.25O2 Catalyst
Surface
Quantum Mechanical DFT Calculations
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DFT COMPUTATIONSCO conversion energetics
CO‐gp
CO‐ads
CO2‐des O2‐gp
O2‐ads
2nd CO‐gp
2nd CO22 CO2 gp
‐200,0
‐180,0
‐160,0
‐140,0
‐120,0
‐100,0
‐80,0
‐60,0
‐40,0
‐20,0
0,01 3 5 7 9 11
Relativ
e En
ergy (kcal/mol)
Pd‐CeZrO2
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The Langmuir Treatment of Adsorption
Ideal Surface Requirements
1. Energetically homogeneous or uniform surface;
2. Energy of interaction with the adsorbate is not affected by the presence or absence of adsorbate on adjoining sites;
3. Each site can accommodate only one adsorbate molecule or atom;
4. Adsorption would occur when an adsorbate molecule or atom with the required energy strikes an unoccupied site;
5. The energy contours would be unaffected by the extent of adsorption;
6. All adsorption has the same mechanism; each has the same structure;
7. The extent of adsorption is less than one complete monolayer
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If ra=Rate of adsorption,
rs= No. of molecules striking the surf./ time-area (bare surf.)
Then ra= s . rs
ra=kaPA(1- θ)
where; ka=Ads. Rate Const.
θ=Fraction occupied by already adsorbed molecules
Also if rd= Rate of desorptionrd=kd θ
At Equilibrium: ra = rd
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If A + S ka
kd
A S (Elementary Step)
with microscopic reversibility, then
and
Introduce Where V=Vol. Adsorbed
Vm= Vol. Adsorbed by all the active sites covered
NOTE: This treatment is applicable to both physical ads. & chemisorption