Fundamental Concepts in Heterogeneous Catalysis
Total Page:16
File Type:pdf, Size:1020Kb
Load more
Recommended publications
-
Surface Reactions and Chemical Bonding in Heterogeneous Catalysis
Surface reactions and chemical bonding in heterogeneous catalysis Henrik Öberg Doctoral Thesis in Chemical Physics at Stockholm University 2014 Thesis for the Degree of Doctor of Philosophy in Chemical Physics Department of Physics Stockholm University Stockholm 2014 c Henrik Oberg¨ ISBN 978-91-7447-893-8 Abstract This thesis summarizes studies which focus on addressing, using both theoretical and experimental methods, fundamental questions about surface phenomena, such as chemical reactions and bonding, related to processes in heterogeneous catalysis. The main focus is on the theoretical approach and this aspect of the results. The included articles are collected into three categories of which the first contains detailed studies of model systems in heterogeneous catalysis. For example, the trimerization of acetylene adsorbed on Cu(110) is measured using vibrational spectroscopy and modeled within the framework of Density Functional Theory (DFT) and quantitative agreement of the reaction barriers is obtained. In the second category, aspects of fuel cell catalysis are discussed. O2 dissociation is rate-limiting for the reduction of oxygen (ORR) under certain conditions and we find that adsorbate-adsorbate interactions are decisive when modeling this reaction step. Oxidation of Pt(111) (Pt is the electrocatalyst), which may alter the overall activity of the catalyst, is found to start via a PtO-like surface oxide while formation of a-PtO2 trilayers precedes bulk oxidation. When considering alternative catalyst materials for the ORR, their stability needs to be investigated in detail under realistic conditions. The Pt/Cu(111) skin alloy offers a promising candidate but segregation of Cu atoms to the surface is induced by O adsorption. -
Insight Into Adsorption Thermodynamics
16 Insight Into Adsorption Thermodynamics Dr. Papita Saha and Shamik Chowdhury Biotechnology Department, National Institute of Technology-Durgapur, Mahatma Gandhi Avenue, Durgapur (WB)-713209 India 1. Introduction Saving the environment to save the Earth and to make the future of mankind safe is the need of the hour. Over the past several decades, the exponential population and social civilization change, affluent lifestyles and resources use, and continuing progress of the industrial and technologies has been accompanied by a sharp modernization and metropolitan growth. The world is reaching new horizons but the cost which we are paying or we will pay in near future is surely going to be high. Among the consequences of this rapid growth is environmental disorder with a big pollution problem. Rapid industrialization, unplanned urbanization and unskilled utilization of natural water resources have led to the destruction of water quality in many parts of the world. In many developing countries, groundwater provides drinking water for more than one-half of the nation's population, and is the sole source of drinking water for many rural communities and some large cities. However, due to industrial, agricultural and domestic activities, a variety of chemicals can pass through the soil and potentially contaminate natural water resources and reservoirs. In recent years, the surge of industrial activities has led to tremendous increase in the use of heavy metals, synthetic dyes and other toxic chemicals, and inevitably resulted in an increased flux of these substances in the aquatic environment. Environmental contamination by toxic heavy metals and synthetic dyes is becoming a serious dilemma now days due to their negative ecotoxicological effects and bioaccumulation in wildlife. -
High Pressure Hydrogen Sorption Isotherms on Microporous Fluorinated Metal Organic Frameworks (FMOF) and BPL Carbon Using High‐Pressure TGA (TGA‐HP)
High Pressure Hydrogen Sorption Isotherms on Microporous Fluorinated Metal Organic Frameworks (FMOF) and BPL Carbon Using High‐Pressure TGA (TGA‐HP) Qian Mather and A. F. Venero TA Instruments‐Waters LLC, 159 Lukens Drive, New Castle, DE 19720, USA Prof. Mohammad Omary, University of North Texas, Denton, TX, USA ABSTRACT This paper discusses the use of high‐pressure TGA (TGA‐HP) to investigate the hydrogen storage capacity of a novel fluorinated metal organic framework (FMOF). INTRODUCTION Hydrogen is attractive as the clean energy source of the future and as a potential replacement for fossil fuels due to the absence of harmful exhaust emissions and compatibility with fuel cells. The challenge for adopting hydrogen as a fuel source is the need for practical, portable storage systems.1 Potential hydrogen storage technologies include containers of compressed or liquefied H2, carbon nanotubes, metal hydrides and metal organic frameworks (MOFs), which store hydrogen via physisorption or chemisorption. The Department of Energy (DOE) has set aggressive targets for hydrogen storage capacity at near‐ambient temperatures and pressures. At present, none of the currently‐available candidate storage materials possess the combination of high hydrogen densities, low desorption temperatures, fast kinetics, and low‐cost needed for automotive applications that meet the DOE criteria. Recently, new microporous metal‐ organic frameworks (MOFs) were found to be promising candidates for hydrogen storage. Porous MOFs are constructed through the assembly of metal‐containing clusters with multidentate organic ligands via coordination bonds into a three‐dimensional structure with well‐defined pore size and morphology. Because of their high surface area, controlled pore size and functionality, high gas sorption capacities are observed. -
The Kinetics of Elementary Thermal Reactions in Heterogene- Ous Catalysis
1 The kinetics of elementary thermal reactions in heterogene- 2 ous catalysis 3 G. Barratt Park1,2, Theofanis Kitsopoulos2,5,6, Dmitriy Borodin1, Kai Golibrzuch2, Jannis 4 Neugebohren1, Daniel J. Auerbach2, Charles T. Campbell4 & Alec M. Wodtke1,2,3* 5 1Institute for Physical Chemistry, Georg-August University of Goettingen, Tammannstraße 6, 6 37077 Göttingen, Germany. 7 2Department of Dynamics at Surfaces, Max Planck Institute for Biophysical Chemistry, Am 8 Faßberg 11, 37077 Göttingen, Germany. 9 3International Center for Advanced Studies of Energy Conversion, Georg-August University 10 of Goettingen, Tammannstraße 6, 37077 Göttingen, Germany. 11 4 Department of Chemistry, University of Washington, Seattle, WA 98195-1700, USA 12 5 Department of Chemistry, University of Crete, Heraklion, Greece 13 6 Institute of Electronic Structure and Laser – FORTH, Heraklion, Greece 14 15 *email: [email protected] 16 17 KEYWORDS: Ion-imaging, velocity-resolved kinetics, CO oxidation, heterogeneous catalysis, 18 slice ion-imaging, molecular beams, surface chemistry. 19 20 1 21 Abstract 22 The kinetics of elementary reactions is fundamental to our understanding of catalysis. Just as 23 micro-kinetic models of atmospheric chemistry provided the predictive power that led to the 24 Montreal protocol reversing loss of stratospheric ozone, pursuing a micro-kinetic approach to 25 heterogeneous catalysis has tremendous potential for societal impact. However, developing this 26 approach for catalysis faces great challenges. Methods for measuring rate constants are quite 27 limited and present predictive theoretical methods remain largely un-validated. This paper pre- 28 sents a short perspective on recent experimental advances in our ability to measure the rates of 29 elementary reactions at surfaces that rely on a stroboscopic pump-probe concept for neutral 30 matter. -
Chemisorption Poster
Chemisorption Presented by Micromeritics Instrument Corporation Blue spheres: Red spheres: Red and Green: surface molecules gas molecules molecules react only with hemisorption: Chemical 1.) 2.) 3.) each other to form a new adsorption is an interaction Green spheres: molecular species muchC stronger than physical ad- active sites sorption. In fact, the interaction is an actual chemical bond where electrons are shared between the gas and the solid surface. While physical adsorption takes place on all surfaces if temperature and pressure conditions are favorable, chemisorption only occurs on cer- tain surfaces and only if these sur- faces are clean. Chemisorption, unlike physisorption, ceases when the adsorbate can no longer make direct contact with the surface; it is therefore a single layer process. Most medicinal, chemical, and petroleum-derived items in Chemisorption Physisorption Many molecules must be activated before they will react ac- common usage are dependent at some stage in their manu- cording to present theories. Activation energy is a measure Near or above dew point Temperature Range: Unlimited facture on a heterogeneous catalytic process. High octane of gas of the energy which must be supplied to them to bring about gasoline, plastics, fertilizers, and herbicides would either be reaction. In some cases the activation energy requirement is prohibitively expensive or unobtainable without them. Like- Enthalpy of Typically Typically such that reaction will proceed only at a measurable rate above (5 - 80 kJ/mol) wise, pollution control would be almost nonexistent were it Adsorption: (80 - 800 kJ/mol) a certain temperature. In others, reaction proceeds rapidly at not for catalysts. Nature of the low temperature, hydrogen on platinum being an example of a Irreversible Reversable adsorption: chemisorption reaction where the activation energy approach- Physical and Chemical Limited to one es zero. -
Elucidating CO2 Chemisorption in Diamine-Appended Metal–Organic Frameworks Alexander C
Elucidating CO2 Chemisorption in Diamine-Appended Metal–Organic Frameworks Alexander C. Forse,a,b,d Phillip J. Milner,a,e,† Jung-Hoon Lee,c,f Halle N. Redfearn,a Julia Oktawiec,a Rebecca L. Siegelman,a,e Jeffrey D. Martell,a Bhavish Dinakar,b,e Leo B. Porter-Zasada,a Miguel I. Gonzalez,a Jeffrey B. Neaton,*c,f,g Jeffrey R. Long,*a,b,e Jeffrey A. Reimer*b,e aDepartment of Chemistry, bDepartment of Chemical and Biomolecular Engineering, cDepartment of Physics, and dBerkeley Energy and Climate Institute, University of California, Berkeley, California 94720, U.S.A. eMaterials Sciences Division, Lawrence Berkeley National Laboratory, Berkeley, California 94720, U.S.A. fMolecular Foundry, Lawrence Berkeley National Laboratory, Berkeley, California 94720, U.S.A. gKavli Energy Nanosciences Institute at Berkeley, Berkeley, California 94720, U.S.A. ABSTRACT: The widespread deployment of carbon capture and sequestration as a climate change mitigation strategy could be facilitated by the development of more energy-efficient adsorbents. Diamine-appended metal–organic frameworks of the type diamine–M2(dobpdc) (M = Mg, Mn, Fe, Co, Ni, Zn; dobpdc4− = 4,4′-dioxidobiphenyl-3,3′-dicarboxylate) have shown promise for carbon capture applications, although questions remain regarding the molecular mechanisms of CO2 uptake in these materials. Here, we leverage the crystallinity and tunability of this class of frameworks to perform a comprehensive study of CO2 chemisorption. Using multinuclear nuclear magnetic resonance (NMR) spectroscopy experiments and van der Waals-corrected density functional theory (DFT) calculations for thirteen diamine–M2(dobpdc) vari- ants, we demonstrate that the canonical CO2 chemisorption products—ammonium carbamate chains and carbamic acid pairs—can be readi- ly distinguished, and that ammonium carbamate chain formation dominates for diamine–Mg2(dobpdc) materials. -
I IMPROVING PALLADIUM CATALYSIS with SELF
IMPROVING PALLADIUM CATALYSIS WITH SELF-ASSEMBLED MONOLAYERS by STEPHEN T. MARSHALL B.S., Carnegie Mellon University, 2005 A thesis submitted to the Faculty of the Graduate School of the University of Colorado in partial fulfillment of the requirement for the degree of Doctor of Philosophy Department of Chemical and Biological Engineering 2010 i This thesis entitled: Improving Palladium Catalysis with Self-Assembled Monolayers written by Stephen T. Marshall has been approved for the Department of Chemical and Biological Engineering J. William Medlin John L. Falconer Date The final copy of this thesis has been examined by the signatories, and we Find that both the content and the form meet acceptable presentation standards Of scholarly work in the above mentioned discipline. ii ABSTRACT Marshall, Stephen T. (Ph.D., Chemical and Biological Engineering) Improving Palladium Catalysis with Self-Assembled Monolayers Thesis directed by Associate Professor J. William Medlin Improving selectivity in catalytic systems is of primary interest to a number of fields. One means of achieving selectivity is through the use of promoters, or deposited materials that improve catalytic properties. Here, we present the modification of palladium surfaces with self- assembled monolayers (SAMs) formed from thiols. SAM coatings are employed in two systems: metal-insulator-semiconductor (MIS) sensors and supported palladium catalysts. On MIS sensors, modification with alkanethiol SAMs results in enhanced sensitivity to acetylene. Excellent selectivity for acetylene over ethylene is also observed. The functionalized sensors would serve as excellent acetylene detectors in a variety of applications including the detection of fault gases in transformers and detecting trace acetylene in ethylene production plants. -
Chemistry of Acetylene on Platinum (111) and (100) Surfaces (Chemisorption/Ultra-High Vacuum/Metal Surface Chemistry/Hydrocarbon Reactions) E
Proc. Nati Acad. Sci. USA Vol. 78, No. 11, pp. 6571-6575, November 1981 Chemistry Chemistry of acetylene on platinum (111) and (100) surfaces (chemisorption/ultra-high vacuum/metal surface chemistry/hydrocarbon reactions) E. L. MUETTERTIESt, M.-C. TSAit, AND S. R. KELEMENt tMaterials and Molecular Research Division, Lawrence Berkeley Laboratory, Berkeley, California 94720; and Department of Chemistry, University of California, Berkeley, California 94720; and tCorporate Research Science Laboratories, Exxon Research and Engineering Company, P.O. Box 45, Linden, New Jersey 07036 Contributed by Earl L. Muetterties, July 24, 1981 ABSTRACT An ultra-high vacuum experimental study of face generated showed the 5 x 20 low energy electron diffiac- acetylene chemisorption on Pt(111) and Pt(100) and ofthe reaction tion pattern. The 5 X 20 surface converted to the 1 X 1 structure of hydrogen with the acetylene adsorbate has established distin- with exposure to acetylene (5). The 1 x 1 surface is stabilized guishing features ofcarbon-hydrogen bond breaking and making by the presence of acetylene and is present during the hydro- processes as a function ofpressure, temperature, and surfacecrys- genation and dehydrogenation processes discussed in this tallography. The rates for both processes are substantially higher article. on the Pt(100) surface. Net acetylene-hydrogen processes, in the temperature range of20°C to -13rC, are distinctly different on the two surfaces: on Pt(100) the net reaction is hydrogen exchange RESULTS ('H. H exchange) and on Pt(III) the only detectable reaction is hydrogenation. Stereochemical differences in the acetylene ad- Acetylene is the simplest unsaturated hydrocarbon. Its geo- sorbate structure are considered to be a contributing factor to the metric structure, electronic structure, and organic chemistry differences in acetylene chemistry on these two surfaces. -
PDF (Chapter 5
~---=---5 __ Heterogeneous Catalysis 5.1 I Introduction Catalysis is a term coined by Baron J. J. Berzelius in 1835 to describe the property of substances that facilitate chemical reactions without being consumed in them. A broad definition of catalysis also allows for materials that slow the rate of a reac tion. Whereas catalysts can greatly affect the rate of a reaction, the equilibrium com position of reactants and products is still determined solely by thermodynamics. Heterogeneous catalysts are distinguished from homogeneous catalysts by the dif ferent phases present during reaction. Homogeneous catalysts are present in the same phase as reactants and products, usually liquid, while heterogeneous catalysts are present in a different phase, usually solid. The main advantage of using a hetero geneous catalyst is the relative ease of catalyst separation from the product stream that aids in the creation of continuous chemical processes. Additionally, heteroge neous catalysts are typically more tolerant ofextreme operating conditions than their homogeneous analogues. A heterogeneous catalytic reaction involves adsorption of reactants from a fluid phase onto a solid surface, surface reaction of adsorbed species, and desorption of products into the fluid phase. Clearly, the presence of a catalyst provides an alter native sequence of elementary steps to accomplish the desired chemical reaction from that in its absence. If the energy barriers of the catalytic path are much lower than the barrier(s) of the noncatalytic path, significant enhancements in the reaction rate can be realized by use of a catalyst. This concept has already been introduced in the previous chapter with regard to the CI catalyzed decomposition of ozone (Figure 4.1.2) and enzyme-catalyzed conversion of substrate (Figure 4.2.4). -
Heterogeneous Catalysis on Metal Oxides
catalysts Review Heterogeneous Catalysis on Metal Oxides Jacques C. Védrine ID Laboratoire de Réactivité de Surface, Université P. & M. Curie, Sorbonne Université, UMR-CNRS 7197, 4 Place Jussieu, F-75252 Paris, France; [email protected]; Tel.: +33-1-442-75560 Received: 8 October 2017; Accepted: 27 October 2017; Published: 10 November 2017 Abstract: This review article contains a reminder of the fundamentals of heterogeneous catalysis and a description of the main domains of heterogeneous catalysis and main families of metal oxide catalysts, which cover acid-base reactions, selective partial oxidation reactions, total oxidation reactions, depollution, biomass conversion, green chemistry and photocatalysis. Metal oxide catalysts are essential components in most refining and petrochemical processes. These catalysts are also critical to improving environmental quality. This paper attempts to review the major current industrial applications of supported and unsupported metal oxide catalysts. Viewpoints for understanding the catalysts’ action are given, while applications and several case studies from academia and industry are given. Emphases are on catalyst description from synthesis to reaction conditions, on main industrial applications in the different domains and on views for the future, mainly regulated by environmental issues. Following a review of the major types of metal oxide catalysts and the processes that use these catalysts, this paper considers current and prospective major applications, where recent advances in the science -
Gold Catalysts Containing Interstitial Carbon Atoms Boost Hydrogenation Activity
ARTICLE https://doi.org/10.1038/s41467-020-18322-x OPEN Gold catalysts containing interstitial carbon atoms boost hydrogenation activity Yafei Sun1,6, Yueqiang Cao 2,6, Lili Wang1,6, Xiaotong Mu1, Qingfei Zhao1, Rui Si3, Xiaojuan Zhu1, ✉ Shangjun Chen1, Bingsen Zhang 4, De Chen5 & Ying Wan 1 Supported gold nanoparticles are emerging catalysts for heterogeneous catalytic reactions, including selective hydrogenation. The traditionally used supports such as silica do not favor 1234567890():,; the heterolytic dissociation of hydrogen on the surface of gold, thus limiting its hydrogenation activity. Here we use gold catalyst particles partially embedded in the pore walls of meso- porous carbon with carbon atoms occupying interstitial sites in the gold lattice. This catalyst allows improved electron transfer from carbon to gold and, when used for the chemoselective hydrogenation of 3-nitrostyrene, gives a three times higher turn-over frequency (TOF) than that for the well-established Au/TiO2 system. The d electron gain of Au is linearly related to the activation entropy and TOF. The catalyst is stable, and can be recycled ten times with negligible loss of both reaction rate and overall conversion. This strategy paves the way for optimizing noble metal catalysts to give an enhanced hydrogenation catalytic performance. 1 Key Laboratory of Resource Chemistry of Ministry of Education, Shanghai Key Laboratory of Rare Earth Functional Materials, and Department of Chemistry, Shanghai Normal University, 200234 Shanghai, China. 2 State Key Laboratory of Chemical Engineering, East China University of Science and Technology, 200237 Shanghai, China. 3 Shanghai Synchrotron Radiation Facility, Shanghai Institute of Applied Physics, Chinese Academy of Sciences, 201204 Shanghai, China. -
N76-21508 Introduction
PHOTOCATALYTIC GENERATION OF HYDROGEN FROM WATER W.R. Bottoms and R.B. Miles Princeton University N76-21508 INTRODUCTION The dissociation of simple molecules provides a potentially efficient method of storing energy in a transportable form. Among the numerous chemical systems that have been proposed for energy conversion are the following: hv 2NOC1 ™ C\2 + 2NO hi> 2H20 ^ 2H2 + 02 2CO2 ^ 2CO + O2 Hydrogen offers the advantages of being a clean burning fuel, easily stored in gas, liquid, or hydride form, and efficiently transferable. It may be used as a fuel for a variety of energy conversion processes including fuel cells and rocket engines as well as conventional heat engines. In conjunction with a water dissociation process, it holds forth the promise of providing a closed cycle, photon powered, energy system where photon energy may be efficiently stored for future use and converted to thermal or electrical energy on demand. In this paper we will discuss a new concept which is designed to overcome the problems encountered when using photodissociation for the generation of hydrogen. Two fundamental problems limiting the efficiency of photodissociation of water are the separation of the photolysis products and the high energy photons necessary for the reaction. Although there has not been a great deal of work with metal-water systems, it has been shown that the dissociation energy of a large number of molecules is catalytically reduced when these molecules are in intimate contact with a surface of certain metals (ref. 1). The spontaneous dissociation of water has been demonstrated for Cu (ref. 2), Fe (ref.