DOCSLIB.ORG

Supporting Information for Hydrogen Chemisorption Isotherms on Pt Particles at Catalytic Temperatures: Langmuir and Two-Dimensional Gas Models Revisited

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
Supporting Information for Hydrogen Chemisorption Isotherms on Pt Particles at Catalytic Temperatures: Langmuir and Two-Dimensional Gas Models Revisited Supporting Information for Hydrogen Chemisorption Isotherms on Pt Particles at Catalytic Temperatures: Langmuir and Two-Dimensional Gas Models Revisited Mónica García-Diéguez,1 David D. Hibbitts,1,2,* and Enrique Iglesia1,3,* 1 Department of Chemical and Biomolecular Engineering, University of California, Berkeley, CA, 94720 2 Department of Chemical Engineering, University of Florida, Gainesville, FL, 32601 3 Division of Chemical Sciences, E.O. Lawrence Berkeley National Laboratory, Berkeley, CA, 94720 * to whom correspondence should be addressed: [email protected], [email protected] S1 Table of Contents Section S1. Details of Standard Statistical Mechanics Treatments S3 Section S2. Derivation of Thermodynamic Treatments S5 Section S3. Adsorption Isotherms S7 Figure S1. S7 Section S4. Temperature Dependence of the Heat of Adsorption and Entropy Loss S8 Section S5. Local Langmuir Isotherm for Non-Uniform Surfaces: QH Approach S12 Table S1. S13 Figure S2. S14 Figure S3. S15 Figure S4. S15 Figure S5. S16 Figure S6. S16 Section S5. Local Langmuir Isotherm for Non-Uniform Surfaces: ΔG Approach S17 Figure S7. S18 Table S2. S19 Table S3. S19 Figure S8. S20 Figure S9. S20 Figure S10. S21 Figure S11. S21 Figure S12. S22 Section S6. Diffusion Barrier—Frustrated Translations S23 Figure S13. S23 Section S7. Detailed DFT Calculation Results S24 Table S4. S24 Table S5. S25 References (Supporting Information). S25 S2 Section S1. Details of Standard Statistical Mechanics Treatments The enthalpy of a given state can be written as the sum of the DFT-derived energy (E0), zero-point vibrational enthalpy (ZPVE) and vibrational, translational and rotational enthalpy (Hvib, Htrans and Hrot): H= E0 + ZPVE + Hvib + H trans + H rot (S1) similarly, the free energy of a state can be written as: G= E0 + ZPVE + Gvib + G trans + G rot (S2) and entropy can be determined for a state with a known H and G at a given T: HG− S = (S3) T For calculations which include a periodic Ir(111) surface (including adsorbed species and transition states on that surface), there are no translational or rotational degrees of freedom and DFT-derived vibrational frequencies can be used to determine the ZPVE, Hvib and Gvib shown in Eqns. S4-6. 푍푃푉퐸 = ∑(½휈ℎ) (S4) −휈ℎ 휈 ℎ푒 푘푇 퐻 = ∑ ( ) (S5) 푣푏 −휈ℎ 1−푒 푘푇 1 퐺 = ∑ (−푘푇 ln ) (S6) 푣푏 −휈ℎ 1−푒 푘푇 Gas-phase molecules have translational and rotational degrees of freedom; thus Htrans, Hrot, Gtrans and Grot must also be computed: 5 퐻푡푟푎푛푠 = ⁄2 푘푇 (S7) 퐻푟표푡,푙푛푒푎푟 = 푘푇 (S8) 3 퐻푟표푡,푛표푛푙푛푒푎푟 = ⁄2 푘푇 (S9) S3 2휋푀푘푇 3⁄2 퐺 = −푘푇 ln [( ) 푉] (S10) 푡푟푎푛푠 ℎ2 1⁄2 휋1⁄2 푇3 퐺푟표푡 = −푘푇 ln [ ( ) ] (S11) 휎 휃푥휃푦휃푧 ℎ2 휃 = 2 (S12) 8휋 퐼푘 where Ii is the moment of inertia about axes x, y or z and σ is the symmetry number of the molecule, 2 for H2. S4 Section S2. Derivation of Thermodynamic Treatments The surface area (퐴surf) of the two-dimensional adsorbed phase is constant (analogous to a constant volume in a three-dimensional system), and therefore the enthalpy is identical to the internal energy (H = U) and the Gibb’s free energy is identical to the Helmholtz free energy (G = A). 퐺 = 퐴 = −푘퐵푇 ln 푄 (S13) Entropy can be obtained from the Helmholtz free energy via a Maxwell relation: 휕퐴 푆 = − ) (S14) 휕푇 푁,퐴surf For identical non-interacting classical particles, we can describe the single-particle partition function (q) in a two- dimensional potential energy surface as: −퐸(푥,푦) 1 ( ) 푘퐵푇 푞 = 2 ∬ 푒 푑푥푑푦 (S15) Λ푡ℎ The integral above is done over the entire metal surface (퐴surf) and 퐸(푥, 푦) ≥ 0, therefore the integral has a maximum value of 퐴surf. Let’s define (to make things simpler), the area from the PES per surface metal atom as 훼푃퐸푆: −퐸(푥,푦) −퐸(푥,푦) 1 ( ) ( ) 푘 푇 푘푇 훼푃퐸푆 = ∬ 푒 퐵 푑푥푑푦 = ∬ 푒 푑푥푑푦 (S16) 푁Msurf 1×1 Note: If the potential energy surface is flat, then 훼푃퐸푆 is the area of a 1×1 Pt (111) surface. The total canonical partition function is: 푞푁 푄 = (S17) 푁! and we can substitute Eq. S15 into that, and apply Stirling’s approximation, to get: 푁 푁 푁 푁 푁 훼푃퐸푆푁Msurf푒 훼푃퐸푆푒 푄 = 2푁 푁 = 2푁 푁 (S18) Λ푡ℎ 푁 Λ푡ℎ 휃 where N is the number of H* adsorbates and θ is the ratio of H* to surface-metal atoms. Substituting the expression for Q into Eq. S17. 푥푦 푥푦 훼푃퐸푆 퐺H*,avg,PES = 퐴H*,avg,PES = −푅푇 [ln ( 2 ) + 1] (S19) Λ푡ℎ휃 Before defining the entropy, I will put the definition of α back in. The average (or integral) molar translational free energy of a species with a given potential energy surface, 퐸(푥, 푦), is: −퐸(푥,푦) 1 ( ) 푥푦 푥푦 푘푇 퐺H*,avg,PES = 퐴H*,avg,PES = −푅푇 [푙푛 ( 2 ∬ 푒 푑푥푑푦) + 1] (S20) Λ푡ℎ휃 1×1 where we will bound the integral within a 1 × 1 surface. Differentiation gives: 푥푦 휕퐴H*,avg,PES 푆푥푦 = − ) (S21) H*,avg,PES 휕푇 퐴,푁 −퐸(푥,푦) 퐸(푥, 푦) ( ) −퐸(푥,푦) 푘푇 1 ( ) ∬ 푒 푑푥푑푦 푥푦 푘푇 1×1 푘푇 푆H*,avg,PES = 푅 [푙푛 ( 2 ∬ 푒 푑푥푑푦) + −퐸(푥,푦) + 2] (S22) Λ 휃 ( ) 푡ℎ 1×1 푘푇 ∬1×1 푒 푑푥푑푦 The other term we will define is a Boltzmann-averaged energy (훽푃퐸푆): S5 −퐸(푥,푦) 퐸(푥, 푦) ( ) 푘푇 훽푃퐸푆 = ∬ 푒 푑푥푑푦 (S23) 1×1 푘푇 Computing the differential free energy and entropies from these average properties gives (and substituting Eqs. S16 and 23 for α and β): 푥푦 훼푃퐸푆 퐺H*,PES = −푅푇푙푛 ( 2 ) (S24) Λ푡ℎ휃 푥푦 훼푃퐸푆 훽푃퐸푆 푆H*,PES = 푅 [푙푛 ( 2 ) + + 1] (S25) Λ푡ℎ휃 훼푃퐸푆 These equations are used as the starting point for determining the two-dimensional translational free energy and entropy for adsorbed H* as further described in the main text. The free energy of a 2-D system described by a PES is given by Eq. S24. For a flat PES (ideal gas), the ‘area’ of the PES (훼푃퐸푆) is the area of each metal atom (훼0): 푥푦 훼0 퐺H*,ideal = −푅푇푙푛 ( 2 ) (S26) Λ푡ℎ휃 In an excluded area model, with an otherwise-flat PES, this area is decreased by the area of a H* atom, when such an atom is present. As such, 훼0 is replaced by (훼0 − 휃푏): 푥푦 훼0 − 휃푏 퐺H*,co-area = −푅푇푙푛 ( 2 ) (S27) Λ푡ℎ휃 Taking the derivative of this free energy term at constant T and N (number of H*) gives the entropy: 푥푦 휕퐺H*,co-area 푆푥푦 = − ) (S28) H*,co-area 휕푇 퐴,푁 gives an expression for the two-dimensional translational entropy of an excluded-area gas model: 푥푦 1 훼0 − 휃푏 푏 푆H*,co-area = 푅 [푙푛 ( 2 ∙ ) + 1 − ] (S29) Λ푡ℎ 휃 훼0 − 휃푏 S6 Section S3. Adsorption Isotherms 1.2 (a) (b) (c) 1.0 H 0.8 θ 0.6 0.4 H* coverage, 0.2 0.0 0.001 0.001 0.001 P (kPa) PH (kPa) PH (kPa) H2 2 2 Figure S1. Adsorption isotherms for H2 dissociative adsorption on Pt (1.6 % wt. Pt/Al2O3 9.1 nm (a) and 3.0 nm (b) mean cluster size; 1 % wt. Pt/SiO2 1.6 nm mean cluster size (c)) at 673 K (), 623 K (), 573 K (▲), 548 (+), 523 K (), 498 K (×) and 473 K (). S7 Section S4. Temperature Dependence of the Heat of Adsorption and Entropy Loss S2.1. Change in enthalpy: The temperature dependence of the isosteric heat of adsorption as a consequence of the change in enthalpy upon H2 dissociative adsorption is given by the difference in heat capacities ( − Cp ) between the gas phase (Cg) and the adsorbate ( Ca ): QH Hg Ha = − 2 = (C − 2Ca ) = −Cp (S30) T T T g p H n where, Hg and Ha are the molar gas-phase enthalpy and the differential adsorbed phase enthalpy, respectively. The isosteric heat of adsorption ( (Q ) ) is related to the differential heat of adsorption (QH) H H by: (Q ) = Q + RT . H H H Local (S31a) and mobile (S31b) dissociative H2 adsorption can be described by the following expressions: 1 2 1 2 2 K P = H H2 K P = H (S31a) H 1+ K 1 2P 1 2 H H2 1− H H2 H 2 = K 1 2P 1 2 or K P = H exp H (S31b) H H H2 H H2 1− H 1− H where P is the hydrogen pressure at equilibrium and KH is the equilibrium constant given in both cases H2 by: E KH = K0 exp (S32) RT in which E is the potential minimum energy of an adsorbed molecule and K0 can be estimated by statistical mechanics as: 2 (qa (T)) K0 (T) = (S33) Qgas (T) qa and Qgas are the molecular partition functions of the adsorbed (H*) and gas (H2) phases, respectively. Substituting Equations (S31a-b), (S32) and (S33) into Equation (4) gives: 2 ln K0 (T) (QH ) = E − RT (S34) H (T) H The partition function for H2 in the gas phase is given by the product of the partition functions for the different degrees of freedom (vibrational (qg,v), translational (qg,t) and rotational (qg,r)): Qgas (T) = qg,vqg,tqg,r (S35) S8 1 exp 2g,v qg,v = (S36a) 1 exp −1 g,v T hg with g,v = and g,v = g,v (2mT)3 2 q = V (S36b) g,t h3 82IT q = = (S36c) g,r h2 g,r τg,v is the vibrational temperature, νg is the vibrational frequency of H2 in the gas phase, h and κ are the Planck’s and Boltzman’s contants, respectively. m is the mass of H2, V is the volume, I is the moment if inertia, σ is the symmetry factor (2 for H2) and τg,v is the rotational temperature.
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.
    [Show full text]
  • 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.
    [Show full text]
  • 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.
    [Show full text]
  • 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.
    [Show full text]
  • 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.
    [Show full text]
  • 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.
    [Show full text]
  • 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).
    [Show full text]
  • 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
    [Show full text]
  • 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.
    [Show full text]
  • Hydrogen Chemisorption Isotherms on Pt Particles at Catalytic
    Article Cite This: J. Phys. Chem. C 2019, 123, 8447−8462 pubs.acs.org/JPCC Hydrogen Chemisorption Isotherms on Platinum Particles at Catalytic Temperatures: Langmuir and Two-Dimensional Gas Models Revisited † † ‡ † § Monicá García-Dieguez,́ David D. Hibbitts,*, , and Enrique Iglesia*, , † Department of Chemical and Biomolecular Engineering, University of California, Berkeley, California 94720, United States ‡ Department of Chemical Engineering, University of Florida, Gainesville, Florida 32601, United States § Division of Chemical Sciences, E. O. Lawrence Berkeley National Laboratory, Berkeley, California 94720, United States *S Supporting Information ABSTRACT: Density functional theory (DFT) and dihydrogen chemisorption uptakes at temperatures relevant to catalysis are used to determine and interpret adsorption enthalpies and entropies over a broad range of chemisorbed hydrogen (H*) coverages (0.1 ML to saturation) on Pt nanoparticles (1.6, 3.0, and 9.1 nm mean diameters) and Pt(111) surfaces. Heats of adsorption decrease by 30 kJ mol−1 ∼ as H2 coverage increases from nearly bare (0.1 ML) to saturated ( 1 ML) surfaces, because of the preferential saturation of low- coordination surface atoms by H* at low coverages. Such surface nonuniformity also leads to stronger binding on small Pt particles at all coverages (e.g., 47 kJ mol−1 on 1.6 nm, 40 kJ mol−1 on 3.0 nm, and 37 kJ mol−1 on 9.1 nm particles all at 0.5 ML), because their surfaces expose a larger fraction of low-coordination atoms. As H* approaches monolayer coverages, H*−H* repulsion leads to a sharp decrease in binding energies on all Pt particles. Measured H* entropies decrease with increasing H* coverage and decreasing particle size, but their values (35−65 J mol−1 K−1) are much larger than for immobile H* species at all coverages and particle sizes.
    [Show full text]
  • Chemical Functionalization of Graphene with Defects
    Chemical functionalization of graphene with defects D. W. Boukhvalov and M. I. Katsnelson Institute for Molecules and Materials, Radboud University Nijmegen, Heyendaalseweg 135, 6525 AJ Nijmegen, The Netherlands Abstract Defects change essentially not only electronic but also chemical properties of graphene being centers of its chemical activity. Their functionalization is a way to modify electronic and crystal structure of graphene which may be important for graphene-based nanoelectronics. Using hydrogen as an example, we have simulated a chemistry of imperfect graphene for a broad class of defects (Stone-Wales defects, bivacancy, nitrogen substitution impurity, and zigzag edges) by density functional calculations. We have studied also an effect of finite width of graphene nanoribbons on their chemical properties. It is shown that magnetism at graphene edges is fragile with respect to oxidation and, therefore, a chemical protection of the graphene edges may be required for application of graphene in spintronics. At the same time, hydrogenation of the Stone-Wales defects may be a perspective way to create magnetic carbon. Graphene [1, 2, 3] is a novel and very perspective material for nanoelectronics [1, 4]. Effect of various imperfections of the crystal lattice, such as Stone-Wales defects (SW) [5], vacancies [6], substitution atoms [7, 8], etc., on physical properties of graphene was studied theoretically [10, 11, 12, 13]. Recently, first experimental observations of defects in graphene have been reported [14, 15, 16]. Earlier, the defects in carbon nanotubes have been intensively investigated [17, 18, 19, 20, 21]. It is known that defects can influence essentially on chemistry of graphene, and there are several theoretical considerations of chemical functionalization of imperfect graphene [12, 22, 23]; also, the defects were experimentally used as attractors for impurities [15].
    [Show full text]
  • Introduction to Chemical Adsorption Analytical Techniques and Their Applications to Catalysis Paul A
    MIC Technical Publications January 2003 Introduction to Chemical Adsorption Analytical Techniques and their Applications to Catalysis Paul A. Webb Micromeritics Instrument Corp., Norcross, Georgia 30093 Abstract The chemical adsorption isotherm reveals information about the active surface of a material and has been em- ployed for many years as a standard analytical tool for the evaluation of catalysts. Temperature-programmed reac- tion techniques have emerged from the 1950’s as an indispensable companion to chemisorption isotherm analyses in many areas of industry and research. This paper provides an introduction to these analytical techniques. Keywords: chemical adsorption, temperature programmed reactions, TPD, TPR, TPO, catalyst 1. Introduction and 800 kJ/mole for chemical bonds. A chemical Optimum design and efficient utilization of cata- bond involves sharing of electrons between the ad- lysts require a thorough understanding of the surface sorbate and the adsorbent and may be regarded as the structure and surface chemistry of the catalytic mate- formation of a surface compound. Due to the bond rial. Chemical adsorption (chemisorption) analyses strength, chemical adsorption is difficult to reverse. can provide much of the information needed to Physical adsorption takes place on all surfaces evaluate catalyst materials in the design and produc- provided that temperature and pressure conditions are tion phases, as well as after a period of use. The re- favorable. Chemisorption, however, is highly selec- quired analytical equipment can be relatively inex- tive and occurs only between certain adsorptive and pensive, simple to operate, and fast compared to al- adsorbent species and only if the chemically active ternate equipment capable of obtaining the same in- surface is cleaned of previously adsorbed molecules.
    [Show full text]