W. F. SchneiderCBE 40445 CBE 40445 Lecture 15 Introduction to Catalysis William F. Schneider Department of Chemical and Biomolecular Engineering Department.

Slides:



Advertisements
Similar presentations
Kinetics of Complex Reactions
Advertisements

Lecture 20. Adsorption Phenomena
Heterogeneous Catalysis & Solid State Physics Dohyung Kim May 2, 2013 Physics 141A.
Adsorption and Catalysis Dr. King Lun Yeung Department of Chemical Engineering Hong Kong University of Science and Technology CENG 511 Lecture 3.
Catalysis and Catalysts - Physical Adsorption Physical Adsorption  Texture and morphology –pore size –pore shape –pore-size distribution (same size or.
“ !” completely different mechanisms. catalysis: the process by which a catalyst changes the rate and mechanism of a chemical reaction -- a catalyst is…
Preparation of catalysts - ExercisesDalian, March-April 20121/xx DICP Course - Dalian, 2012 Preparation of solid catalysts Exercises Supported by the Chinese.
ADSORPTION by Pranoy Pratik Raul.
Intermolecular Forces and
Bonding to surfaces Two classifications distinguished by the magnitude of their enthalpies of adsorption  Physisorption: long-range but weak van der Waals-type.
Electrochemistry for Engineers LECTURE 6 Lecturer: Dr. Brian Rosen Office: 128 Wolfson Office Hours: Sun 16:00.
By: Lance Hammell. What are catalysts? Simply put, catalysts are substances which, when added to a reaction, increase the rate of reaction by providing.
Catalysis for Chemical Engineers
1 Catalyst Fundamentals 朱信 Hsin Chu Professor Dept. of Environmental Eng. National Cheng Kung University.
Catalysts. Syllabus Statements C.4.1 Compare the modes of action of homogeneous and heterogeneous catalysts. C.4.2 Outline the advantages and disadvantages.
Summary comments on mechanism For a reaction mechanism to be viable, two main conditions apply. 1. The sum of the elementary steps must lead to the overall.
INTRODUCTION TO CATALYSIS –KINETICS OF CATALYTIC REACTIONS CH
Introduction to catalysis chemistry
88 ITK-329 Kinetika & Katalisis Introduction to Catalyst & Catalysis Dicky Dermawan Chapter 5.
Heterogeneous catalysis
Chapter 13 Ch 13 Page Chemical Reactions Process Dynamics Abstract concept (orange to clear) Molecules – Have a size and shape. – Have distributions.
Intermolecular Forces and Liquids and Solids Chapter 11.
W. F. SchneiderCBE CBE Lecture 15 Introduction to Catalysis Developed by Prof. Schneider 1,2 Modified by Prof. Hicks 1 1 Department of Chemical.
PE333 Chemical reaction &industrial catalysis (Part 2) Dr/Marwa Abdelfattah Fall
Temperature dependence of reaction rates
Chapter 2 Chemical Reactor Analysis and Design
Chemistry. Surface Chemistry - 1 Session Session Objectives  Adsorption versus absorption  Types of adsorption: physisorption and chemisorption  Desorption.
1 Intermolecular Forces and Liquids and Solids Chapter 12 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Intermolecular Forces and Liquids and Solids Chapter 14.
The final saga.  There is an activation energy for each elementary step.  Activation energy determines k.  k = Ae - (E a /RT)  k determines rate 
Adsorption. What is Adsorption? Adsorption is the transfer of a material from one liquid or gaseous state to a surface. The substance that is transferred.
Nanochemistry NAN 601 Dr. Marinella Sandros
A + B C + D Exothermic Reaction Endothermic Reaction
Kinetics of Complex Reactions
PC4259 Chapter 4 Adsorption on Solid Surfaces & Catalysis
Catalyst Design and Preparation Dr. King Lun Yeung Department of Chemical Engineering Hong Kong University of Science and Technology CENG 511 Lecture 3.
Intermolecular Forces and Liquids and Solids Chapter 10.
Surface and Interface Chemistry  Solid/gas Interface (part two) Valentim M. B. Nunes Engineering Unit of IPT 2014.
Chapter 14 Chemical Kinetics (part 2). The Collision Model Goal: develop a model that explains why rates of reactions increase as concentration and temperature.
Chapter 14 Chemical Kinetics (part 2). The Collision Model Goal: develop a model that explains why rates of reactions increase as concentration and temperature.
Heterogeneous catalysis
§8.5 adsorption at gas / solid interface Levine: pp. 397– 402 section 13.5 adsorption of gases on solids.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemical Kinetics The area of chemistry that concerns reaction rates.
Surface and Interface Chemistry  Solid/gas Interface
Adsorption Modeling of physisorption in porous materials Part 1 European Master Bogdan Kuchta Laboratoire MADIREL Université Aix-Marseille.
Adsorption and Catalysis Dr. King Lun Yeung Department of Chemical Engineering Hong Kong University of Science and Technology CENG 511 Lecture 3.
Industrial catalysis Lec 8 week 11.
Catalysis.
Unit 9 – Reaction Rates and Equilibrium The area of chemistry that concerns reaction rates (how fast a reaction occurs)
H+H+ H+H+ H+H+ OH - New Way Chemistry for Hong Kong A-Level Book 2 1 Chapter 15 The Effect of Temperature Change and Catalyst on Reaction Rate 15.1Effect.
Isotherms and surface reaction mechanisms. 2 Heterogeneous Catalytic Reaction Process  Journey for reactant molecules:  travel within gas phase . cross.
1 Example Heterogeneous Catalytic Reaction Process  The long journey for reactant molecules to .travel within gas phase . cross gas-liquid phase boundary.
Adsorption at solids Solid: Adsorbent Gas/Solute: Adsorbate
Intermolecular Forces and Liquids and Solids Chapter 11 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Collision Theory  Collision theory is a theory proposed independently by Max Trautz in 1916 and William Lewis in 1918, that qualitatively explains how.
S OLID S TATE AND S URFACE C HEMISTRY ( LECTURE 10) Dr. Saeda Rwede Al-Mhyawi Assistant professor in physical chemistry Contact Info:
Aerosol & Particulate Research Lab
Characterization Techniques
AP CHEMISTRY Chapter 14 Chemical Kinetics Chemical Kinetics Study of how rapidly a reaction will occur. In addition to speed of reaction, kinetics.
ADSORPTION The removal of dissolved substances from solution using adsorbents such as activated carbon.
HETEROGENOUS CATALYST
Catalytic Reaction Engineering Catalysis and Catalytic Reactors
School for PhD June 8-12, 2015 Luigi PASQUA
Adsorption and Catalysis
Adsorption 2018/7/1.
Catalysis and Heterogeneous Catalysis
ERT 313 BIOSEPARATION ENGINEERING ADSORPTION
CBE Lecture 15 Introduction to Catalysis
CBE Lecture 15 Introduction to Catalysis
catalysis: the process by which a catalyst changes the
Presentation transcript:

W. F. SchneiderCBE CBE Lecture 15 Introduction to Catalysis William F. Schneider Department of Chemical and Biomolecular Engineering Department of Chemistry and Biochemistry University of Notre Dame Fall Semester 2005

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE What is a “Catalyst” A catalyst (Greek: καταλύτης, catalytēs) is a substance that accelerates the rate of a chemical reaction without itself being transformed or consumed by the reaction. (thank you Wikipedia)Greekratechemical reaction A + B C ΔGΔG EaEa uncatalyzed A + B + catalyst C + catalyst ΔGΔG Ea′Ea′ catalyzed k(T) = k 0 e -Ea/RT E a ′ < E a k 0 ′ > k 0 k′ > k ΔG = ΔG

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Catalysts Open Up New Reaction Pathways CH 3 C O CH 2 C CH 3 OH propanone propenol H2CH2C HO C CH 3 ‡ ‡ propanone propenol

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Catalysts Open Up New Reaction Pathways CH 3 C O CH 2 C CH 3 OH propanone propenol OH − CH 2 C CH 3 O−O− + H 2 O −OH − Base catalyzed propanone propenol intermediate ‡‡ rate = k[OH − ][acetone]

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Catalysts Open Up New Reaction Pathways CH 3 C O CH 2 C CH 3 OH propanone propenol + H 2 O Acid catalyzed H3O+H3O+ CH 3 C OHOH + −H3O+−H3O+ propenol different intermediate ‡‡ propanone rate = k[H 3 O + ][acetone]

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Types of Catalysts - Enzymes The “Gold Standard” of catalysts Highly specific Highly selective Highly efficient Catalyze very difficult reactions  N 2  NH 3  CO 2 + H 2 O  C 6 H 12 O 6 Works better in a cell than in a l reactor Triosephosphateisomerase “TIM” Cytochrome C Oxidase Highly tailored “active sites” Often contain metal atoms

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Types of Catalysts – Organometallic Complexes Perhaps closest man has come to mimicking nature’s success 2005 Noble Prize in Chemistry Well-defined, metal-based active sites Selective, efficient manipulation of organic functional groups Various forms, especially for polymerization catalysis Difficult to generalize beyond organic transformations Polymerization: Termination:

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Types of Catalysts – Homogeneous vs. Heterogeneous Homogeneous catalysis Single phase (Typically liquid) Low temperature Separations are tricky Heterogeneous catalysis Multiphase (Mostly solid-liquid and solid-gas) High temperature Design and optimization tricky Zeolite catalystCatalyst powders

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Types of Catalysts: Crystalline Microporous Catalysts Regular crystalline structure Porous on the scale of molecular dimensions  10 – 100 Å  Up to 1000’s m 2 /g surface area Catalysis through  shape selection  acidity/basicity  incorporation of metal particles 10 Å 100 Å Zeolite (silica-aluminate) Silico-titanate MCM-41 (mesoporous silica)

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Types of Catalysts: Amorphous Heterogeneous Catalysts Amorphous, high surface area supports  Alumina, silica, activated carbon, …  Up to 100’s of m 2 /g of surface area Impregnated with catalytic transition metals  Pt, Pd, Ni, Fe, Ru, Cu, Ru, … Typically pelletized or on monoliths Cheap, high stability, catalyze many types of reactions Most used, least well understood of all classes SEM micrographs of alumina and Pt/alumina

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Important Heterogeneous Catalytic Processes Haber-Bosch process  N H 2 → 2 NH 3  Fe/Ru catalysts, high pressure and temperature  Critical for fertilizer and nitric acid production Fischer-Tropsch chemistry  n CO + 2n H 2 → (CH 2 ) n + n H 2 O, syn gas to liquid fuels  Fe/Co catalysts  Source of fuel for Axis in WWII Fluidized catalytic cracking  High MW petroleum → low MW fuels, like gasoline  Zeolite catalysts, high temperature combustor  In your fuel tank! Automotive three-way catalysis  NO x /CO/HC → H 2 O/CO 2 /H 2 O  Pt/Rh/Pd supported on ceria/alumina  Makes exhaust 99% cleaner

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Heterogeneous Catalytic Reactors Design goals  rapid and intimate contact between catalyst and reactants  ease of separation of products from catalyst Packed Bed (single or multi-tube) Slurry Reactor Fluidized Bed Catalyst Recycle Reactor

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Automotive Emissions Control System “Three-way” Catalyst CO  CO 2 HC  CO 2 + H 2 O NO x  N 2 Pt, Rh, Pd Alumina, ceria, lanthana, … Most widely deployed heterogeneous catalyst in the world – you probably own one! Monolith reactor

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Length Scales in Heterogeneous Catalysis Mass transport/diffusion Chemical adsorption and reaction

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Characteristics of Heterogeneous Supported Catalysts Surface area:  Amount of internal support surface accessible to a fluid  Measured by gas adsorption isotherms Loading:  Mass of transition metal per mass of support Dispersion:  Percent of metal atoms accessible to a fluid support MMM

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Rates of Catalytic Reactions Pseudo-homogeneous reaction rate  r = moles / volume · time Mass-based rate  r′ = moles / mass cat · time  r′ = r / ρ cat Heterogeneous reactions happen at surfaces Area-based rate  r′′ = moles / area cat · time  r′′ = r′ / SA,SA = area / mass Heterogeneous reactions happen at active sites Active site-based rate  Turn-over frequency TOF = moles / site · time  TOF = r′′ / ρ site TOF (s −1 ) Hetero. cats. ~10 1 Enzymes ~10 6 TOF (s −1 ) Hetero. cats. ~10 1 Enzymes ~10 6

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Adsorption and Reaction at Solid Surfaces Physisorption: weak van der Waals attraction of a fluid (like N 2 gas) for any surface  E ads ~10 – 40 kJ/mol  Low temperature phenomenon  Exploited in measuring gross surface area Chemisorption: chemical bond formation between a fluid molecule (like CO or ethylene) and a surface site  E ads ~ 100 – 500 kJ/mol  Essential element of catalytic activity  Exploited in measuring catalytically active sites

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Comparing Physi- and Chemisorption on MgO(001) CO 2 SO 2 Physisorbed CO 2 -2 kcal mol -1 GGA Chemisorbed SO 2 (“sulfite”) -25 kcal mol -1 GGA SO 3 Chemisorbed SO 3 (“sulfate”) -50 kcal mol -1 GGA MgO(001) supercell Mg O :O: surf : : 2- C OO :O: surf : : 2- S OO : :O: surf : : 2- S OO O Schneider, Li, and Hass, J. Phys. Chem. B 2001, 105, 6972 Calculated from first-principles DFT

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Measuring Concentrations in Heterogeneous Reactions Kinetics Fluid concentrations  Traditionally reported as pressures (torr, atm, bar)  Ideal gas assumption: P j = C j RT Surface concentrations  “Coverage” per unit area n j = moles j / area  Maximum coverage called monolayer 1 ML: n j,max = ~ molecules / cm 2  Fractional coverage θ j = n j / n j,max 0 ≤ θ j ≤ 1 θ j = 1/6 Rate = f(P j,θ j ) Metal particle surface

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Adsorption Isotherms Molecules in gas and surface are in dynamic equilibrium A (g) + M (surface) ↔ M-A Isotherm describes pressure dependence of equilibrium Langmuir isotherm proposed by Irving Langmuir, GE, 1915  (1932 Noble Prize)  Adsorption saturates at 1 monolayer  All sites are equivalent  Adsorption is independent of coverage Site conservation θ A + θ* = 1 + Equilibrium rate ads = rate des

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Using the Langmuir Isotherm Example: CO adsorption on 10% Ru/Al 2 O 100°C P CO (torr) CO ads (μmol/g cat ) n CO,∞ = 2.89 μmol/g cat K =

● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ ● ○ W. F. SchneiderCBE Brunauer-Emmett-Teller Isotherm (BET) Solid Surface ΔH ads ΔH cond ΔH ads / ΔH cond Relaxes Langmuir restriction to single layer adsorption  Monolayer adsorption; multilayer condensation Useful for total surface area measurement  Adsorption of boiling N 2 (78 K)