Transition State Theory for Nonequilibrium Systems with Power
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Rate Constants and Kinetic Isotope Effects for Methoxy Radical Reacting with NO2 and O2 Jiajue Chai, Hongyi Hu, Theodore
Rate Constants and Kinetic Isotope Effects for Methoxy Radical Reacting with NO2 and O2 Jiajue Chai, Hongyi Hu, Theodore. S. Dibble* Department of Chemistry, College of Environmental Science and Forestry, State University of New York, Syracuse, New York 13210, United States Geoffrey. S. Tyndall,* and John. J. Orlando Atmospheric Chemistry Division, National Center for Atmospheric Research, Boulder, Colorado 80307, United States Abstract Relative rate studies were carried out to determine the temperature dependent rate constant ratio k1/k2a: CH3O• + O2 → HCHO + HO2• (R1) CH3O• + NO2 (+M) → CH3ONO2 (+ M) (R2a) over the temperature range 250-333 K in an environmental chamber at 700 Torr using FTIR detection. Absolute rate constants k2 were determined using laser flash photolysis/laser induced fluorescence under the same conditions. The analogous experiments were carried out for the reactions of perdeuterated methoxy radical (CD3O•). Absolute rate constants k2 were in excellent agreement with the recommendations of the JPL Data Evaluation panel. The combined data (i.e., 3 -1 k1/k2 and k2) allow determination of k1 as cm s , corresponding to 1.4 × 10-15 cm3 s-1 at 298 K. The rate constant at 298 K is in excellent agreement with previous work, but the observed temperature dependence is less than previously reported. The deuterium isotope effect, kH/kD, can be expressed in Arrhenius form as The deuterium isotope effect does not appear to be greatly influenced by tunneling, which is consistent with previous theoretical work by Hu and Dibble (Hu, H.; Dibble, T. S., J. Phys. Chem. A 2013, 117, 14230–14242). Keywords: methylnitrite, formaldehyde, methylnitrate, alkoxy radicals, kinetic isotope effect * [email protected], [email protected] 1 I. -
Chapter 9. Atomic Transport Properties
NEA/NSC/R(2015)5 Chapter 9. Atomic transport properties M. Freyss CEA, DEN, DEC, Centre de Cadarache, France Abstract As presented in the first chapter of this book, atomic transport properties govern a large panel of nuclear fuel properties, from its microstructure after fabrication to its behaviour under irradiation: grain growth, oxidation, fission product release, gas bubble nucleation. The modelling of the atomic transport properties is therefore the key to understanding and predicting the material behaviour under irradiation or in storage conditions. In particular, it is noteworthy that many modelling techniques within the so-called multi-scale modelling scheme of materials make use of atomic transport data as input parameters: activation energies of diffusion, diffusion coefficients, diffusion mechanisms, all of which are then required to be known accurately. Modelling approaches that are readily used or which could be used to determine atomic transport properties of nuclear materials are reviewed here. They comprise, on the one hand, static atomistic calculations, in which the migration mechanism is fixed and the corresponding migration energy barrier is calculated, and, on the other hand, molecular dynamics calculations and kinetic Monte-Carlo simulations, for which the time evolution of the system is explicitly calculated. Introduction In nuclear materials, atomic transport properties can be a combination of radiation effects (atom collisions) and thermal effects (lattice vibrations), this latter being possibly enhanced by vacancies created by radiation damage in the crystal lattice (radiation enhanced-diffusion). Thermal diffusion usually occurs at high temperature (typically above 1 000 K in nuclear ceramics), which makes the transport processes difficult to model at lower temperatures because of the low probability to see the diffusion event occur in a reasonable simulation time. -
Eyring Equation
Search Buy/Sell Used Reactors Glass microreactors Hydrogenation Reactor Buy Or Sell Used Reactors Here. Save Time Microreactors made of glass and lab High performance reactor technology Safe And Money Through IPPE! systems for chemical synthesis scale-up. Worldwide supply www.IPPE.com www.mikroglas.com www.biazzi.com Reactors & Calorimeters Induction Heating Reacting Flow Simulation Steam Calculator For Process R&D Laboratories Check Out Induction Heating Software & Mechanisms for Excel steam table add-in for water Automated & Manual Solutions From A Trusted Source. Chemical, Combustion & Materials and steam properties www.helgroup.com myewoss.biz Processes www.chemgoodies.com www.reactiondesign.com Eyring Equation Peter Keusch, University of Regensburg German version "If the Lord Almighty had consulted me before embarking upon the Creation, I should have recommended something simpler." Alphonso X, the Wise of Spain (1223-1284) "Everything should be made as simple as possible, but not simpler." Albert Einstein Both the Arrhenius and the Eyring equation describe the temperature dependence of reaction rate. Strictly speaking, the Arrhenius equation can be applied only to the kinetics of gas reactions. The Eyring equation is also used in the study of solution reactions and mixed phase reactions - all places where the simple collision model is not very helpful. The Arrhenius equation is founded on the empirical observation that rates of reactions increase with temperature. The Eyring equation is a theoretical construct, based on transition state model. The bimolecular reaction is considered by 'transition state theory'. According to the transition state model, the reactants are getting over into an unsteady intermediate state on the reaction pathway. -
Tables of Rate Constants for Gas Phase Chemical Reactions of Sulfur Compounds (1971-1979)
NBSIR 80-2118 Tables of Rate Constants for Gas Phase Chemical Reactions of Sulfur Compounds (1971-1979) Francis Westley Chemical Kinetics Division Center for Thermodynamics and Molecular Science National Measurement Laboratory National Bureau of Standards U.S. Department of Commerce Washington. D.C. 20234 July 1980 Interim Report Prepared for Morgantown Energy Technology Center Department of Energy Morgantown, West Virginia 26505 Fice of Standard Reference Data itional Bureau of Standards ashington, D.C. 20234 c, 2 Jl 1 m * rational bureau 07 STANDARDS LIBRARY NBSIR 80-2118 wov 2 4 1980 TABLES OF RATE CONSTANTS FOR GAS f)Oi Clcc -Ore PHASE CHEMICAL REACTIONS OF SULFUR COMPOUNDS (1971-1979) 1 5 (o lo-z im Francis Westley Chemical Kinetics Division Center for Thermodynamics and Molecular Science National Measurement Laboratory National Bureau of Standards U.S. Department of Commerce Washington, D.C. 20234 July 1980 Interim Report Prepared for Morgantown Energy Technology Center Department of Energy Morgantown, West Virginia 26505 and Office of Standard Reference Data National Bureau of Standards Washington, D.C. 20234 U.S. DEPARTMENT OF COMMERCE, Philip M. Klutznick, Secretary Luther H. Hodges, Jr., Deputy Secretary Jordan J. Baruch, Assistant Secretary for Productivity, Technology, and Innovation NATIONAL BUREAU OF STANDARDS. Ernest Ambler, Director . i:i : a 1* V'.OTf in. te- ?') t aa.‘ .1 J Table of Contents Abstract 1 Introduction 2 Guidelines for the User 4 Table of Arrhenius Parameters for Chemical Reactions of Sulfur Compounds 12 Reactions of: S(Sulfur atom) 12 $2(Sulfur dimer) 20 S0(Sulfur monoxide) 21 S02(Sulfur dioxide 23 S0 (Sulfur trioxide) 28 3 S20(Sul fur oxide^O) ) 29 SH (Mercapto free radical) 29 H2S (Hydroqen sulfide 31 CS (Carbon monosulfide free radical) 32 CS2 (Carbon disulfide) 33 COS (Carbon oxide sulfide) 35 CH^S* ( Methyl thio free radical) 36 CH^SH (Methanethiol ) 36 cy-CF^CF^S (Thiirane) 37 CH^SCF^* (Methyl, (methyl thio)-, free radical) ... -
Classical and Modern Methods in Reaction Rate Theory
J. Phys. Chem. 1988, 92, 3711-3725 3711 loss associated with the transition between states is offset by a For the Re( MQ+)-based complexes an additional complication gain in energy in the intramolecular vibrations (eq 3). to intramolecular electron transfer exists arising from a "flattening" On the other hand, if (AGe,,2 + A0,2) > (AG,,l + A,,,) (Figure of the relative orientations of the two rings of the MQ+ ligand 4B) and nuclear tunneling effects in the librational modes are when it accepts an However, the analysis presented unimportant, intramolecular electron transfer can not occur in here does provide a general explanation for the role of free energy a frozen environment. The situation is the same as in Figure 3A. change in environments where dipole motions are restricted. For Even direct Re(1) - MQ' excitation (process a in Figure 4B) a directed, intramolecular electron transfer such as reaction 1, must either lead to the ground state by emission or to the Re- the change in electronic distribution between states will, in general, (11)-bpy'--based MLCT state by reverse electron transfer: lead to a difference between Ao,l and A0,2. This difference creates a solvent dipole barrier to intramolecular electron transfer. It [ (bpy)Re"(CO) 3( MQ')] 2+* -+ (bpy'-)Re"( CO) 3(MQ')] 2'* follows from eq 4 that if light-induced electron transfer is to occur (5) in a frozen environment, the difference in solvent reorganizational The inversion in the sense of the electron transfer in the frozen energy, A& = bS2- A,,, must be compensated for by a favorable environment is induced energetically by the greater solvent re- free energy change, A(AG) = - AGes,l,as organizational energy for the lower excited state, A0,2 > Ao,l - Aces,~- AGes.2 > Ao-2 - &,I (AGes,2 - AGes,l)* or In a macroscopic sample, a distribution of solvent dipole en- vironments exists around the assembly of ground states. -
Spring 2013 Lecture 13-14
CHM333 LECTURE 13 – 14: 2/13 – 15/13 SPRING 2013 Professor Christine Hrycyna INTRODUCTION TO ENZYMES • Enzymes are usually proteins (some RNA) • In general, names end with suffix “ase” • Enzymes are catalysts – increase the rate of a reaction – not consumed by the reaction – act repeatedly to increase the rate of reactions – Enzymes are often very “specific” – promote only 1 particular reaction – Reactants also called “substrates” of enzyme catalyst rate enhancement non-enzymatic (Pd) 102-104 fold enzymatic up to 1020 fold • How much is 1020 fold? catalyst time for reaction yes 1 second no 3 x 1012 years • 3 x 1012 years is 500 times the age of the earth! Carbonic Anhydrase Tissues ! + CO2 +H2O HCO3− +H "Lungs and Kidney 107 rate enhancement Facilitates the transfer of carbon dioxide from tissues to blood and from blood to alveolar air Many enzyme names end in –ase 89 CHM333 LECTURE 13 – 14: 2/13 – 15/13 SPRING 2013 Professor Christine Hrycyna Why Enzymes? • Accelerate and control the rates of vitally important biochemical reactions • Greater reaction specificity • Milder reaction conditions • Capacity for regulation • Enzymes are the agents of metabolic function. • Metabolites have many potential pathways • Enzymes make the desired one most favorable • Enzymes are necessary for life to exist – otherwise reactions would occur too slowly for a metabolizing organis • Enzymes DO NOT change the equilibrium constant of a reaction (accelerates the rates of the forward and reverse reactions equally) • Enzymes DO NOT alter the standard free energy change, (ΔG°) of a reaction 1. ΔG° = amount of energy consumed or liberated in the reaction 2. -
Eyring Activation Energy Analysis of Acetic Anhydride Hydrolysis in Acetonitrile Cosolvent Systems Nathan Mitchell East Tennessee State University
East Tennessee State University Digital Commons @ East Tennessee State University Electronic Theses and Dissertations Student Works 5-2018 Eyring Activation Energy Analysis of Acetic Anhydride Hydrolysis in Acetonitrile Cosolvent Systems Nathan Mitchell East Tennessee State University Follow this and additional works at: https://dc.etsu.edu/etd Part of the Analytical Chemistry Commons Recommended Citation Mitchell, Nathan, "Eyring Activation Energy Analysis of Acetic Anhydride Hydrolysis in Acetonitrile Cosolvent Systems" (2018). Electronic Theses and Dissertations. Paper 3430. https://dc.etsu.edu/etd/3430 This Thesis - Open Access is brought to you for free and open access by the Student Works at Digital Commons @ East Tennessee State University. It has been accepted for inclusion in Electronic Theses and Dissertations by an authorized administrator of Digital Commons @ East Tennessee State University. For more information, please contact [email protected]. Eyring Activation Energy Analysis of Acetic Anhydride Hydrolysis in Acetonitrile Cosolvent Systems ________________________ A thesis presented to the faculty of the Department of Chemistry East Tennessee State University In partial fulfillment of the requirements for the degree Master of Science in Chemistry ______________________ by Nathan Mitchell May 2018 _____________________ Dr. Dane Scott, Chair Dr. Greg Bishop Dr. Marina Roginskaya Keywords: Thermodynamic Analysis, Hydrolysis, Linear Solvent Energy Relationships, Cosolvent Systems, Acetonitrile ABSTRACT Eyring Activation Energy Analysis of Acetic Anhydride Hydrolysis in Acetonitrile Cosolvent Systems by Nathan Mitchell Acetic anhydride hydrolysis in water is considered a standard reaction for investigating activation energy parameters using cosolvents. Hydrolysis in water/acetonitrile cosolvent is monitored by measuring pH vs. time at temperatures from 15.0 to 40.0 °C and mole fraction of water from 1 to 0.750. -
Wigner's Dynamical Transition State Theory in Phase Space
Wigner’s Dynamical Transition State Theory in Phase Space: Classical and Quantum Holger Waalkens1,2, Roman Schubert1, and Stephen Wiggins1 October 15, 2018 1 School of Mathematics, University of Bristol, University Walk, Bristol BS8 1TW, UK 2 Department of Mathematics, University of Groningen, Nijenborgh 9, 9747 AG Groningen, The Netherlands E-mail: [email protected], [email protected], [email protected] Abstract We develop Wigner’s approach to a dynamical transition state theory in phase space in both the classical and quantum mechanical settings. The key to our de- velopment is the construction of a normal form for describing the dynamics in the neighborhood of a specific type of saddle point that governs the evolution from re- actants to products in high dimensional systems. In the classical case this is the standard Poincar´e-Birkhoff normal form. In the quantum case we develop a normal form based on the Weyl calculus and an explicit algorithm for computing this quan- tum normal form. The classical normal form allows us to discover and compute the phase space structures that govern classical reaction dynamics. From this knowledge we are able to provide a direct construction of an energy dependent dividing sur- face in phase space having the properties that trajectories do not locally “re-cross” the surface and the directional flux across the surface is minimal. Using this, we are able to give a formula for the directional flux through the dividing surface that goes beyond the harmonic approximation. We relate this construction to the flux- flux autocorrelation function which is a standard ingredient in the expression for the reaction rate in the chemistry community. -
Lecture 17 Transition State Theory Reactions in Solution
Lecture 17 Transition State Theory Reactions in solution kd k1 A + B = AB → PK = kd/kd’ kd’ d[AB]/dt = kd[A][B] – kd’[AB] – k1[AB] [AB] = kd[A][B]/k1+kd’ d[P]/dt = k1[AB] = k2[A][B] k2 = k1kd/(k1+kd’) k2 is the effective bimolecular rate constant kd’<<k1, k2 = k1kd/k1 = kd diffusion controlled k1<<kd’, k2 = k1kd/kd’ = Kk1 activation controlled Other names: Activated complex theory and Absolute rate theory Drawbacks of collision theory: Difficult to calculate the steric factor from molecular geometry for complex molecules. The theory is applicable essentially to gaseous reactions Consider A + B → P or A + BC = AB + C k2 A + B = [AB] ╪ → P A and B form an activated complex and are in equilibrium with it. The reactions proceed through an activated or transition state which has energy higher than the reactions or the products. Activated complex Transition state • Reactants Has someone seen the Potential energy transition state? Products Reaction coordinate The rate depends on two factors, (i). Concentration of [AB] (ii). The rate at which activated complex is decomposed. ∴ Rate of reaction = [AB╪] x frequency of decomposition of AB╪ ╪ ╪ K eq = [AB ] / [A] [B] ╪ ╪ [AB ] = K eq [A] [B] The activated complex is an aggregate of atoms and assumed to be an ordinary molecule. It breaks up into products on a special vibration, along which it is unstable. The frequency of such a vibration is equal to the rate at which activated complex decompose. -d[A]/dt = -d[B]/dt = k2[A][B] Rate of reaction = [AB╪] υ ╪ = K eq υ [A] [B] Activated complex is an unstable species and is held together by loose bonds. -
Eyring Equation and the Second Order Rate Law: Overcoming a Paradox
Eyring equation and the second order rate law: Overcoming a paradox L. Bonnet∗ CNRS, Institut des Sciences Mol´eculaires, UMR 5255, 33405, Talence, France Univ. Bordeaux, Institut des Sciences Mol´eculaires, UMR 5255, 33405, Talence, France (Dated: March 8, 2016) The standard transition state theory (TST) of bimolecular reactions was recently shown to lead to a rate law in disagreement with the expected second order rate law [Bonnet L., Rayez J.-C. Int. J. Quantum Chem. 2010, 110, 2355]. An alternative derivation was proposed which allows to overcome this paradox. This derivation allows to get at the same time the good rate law and Eyring equation for the rate constant. The purpose of this paper is to provide rigorous and convincing theoretical arguments in order to strengthen these developments and improve their visibility. I. INTRODUCTION A classic result of first year chemistry courses is that for elementary bimolecular gas-phase reactions [1] of the type A + B −→ P roducts, (1) the time-evolution of the concentrations [A] and [B] is given by the second order rate law d[A] − = K[A][B], (2) dt where K is the rate constant. For reactions proceeding through a barrier along the reaction path, Eyring famous equation [2] allows the estimation of K with a considerable success for more than 80 years [3]. This formula is the central result of activated complex theory [2], nowadays called transition state theory (TST) [3–18]. Note that other researchers than Eyring made seminal contributions to the theory at about the same time [3], like Evans and Polanyi [4], Wigner [5, 6], Horiuti [7], etc.. -
On Rate Constants: Simple Collision Theory, Arrhenius Behavior, and Activated Complex Theory
On Rate Constants: Simple Collision Theory, Arrhenius Behavior, and Activated Complex Theory 17th February 2010 0.1 Introduction Up to now, we haven't said much regarding the rate constant k. It should be apparent from the discussions, however, that: • k is constant at a specific temperature, T and pressure, P • thus, k = k(T,P) (rate constant is temperature and pressure depen- dent) • bear in mind that the rate constant is independent of concentrations, as the reaction rate, or velocity itself is treated explicity to be concen- tration dependent In the following, we will consider how the physical, microscopic detaails of reactions can be reasoned to be embodied in the rate constant, k. 1 Simple Collision Theory Let's consider the following gas-phase elementary reaction: A + B ! Products The reaction rate is straightforwardly: 1 Rate = k[A]α[B]β = k[A]1[B]1 α = 1 β = 1 N N = k A B V = volume V V Recall previous discussions of the total collisional frequency for heteroge- neous reactions: 8kT ∗ ∗ ZAB = σAB nA nB s πµ ∗ NA ∗ NB where the nA = V ; nB = V are number of molecules/particles per unit volume. We can see the following: 8kT NA NB ZAB = σAB s πµ V V k Here we see that the concepts| of collisions{z } from simple kinetic theory can be fundamentally related to ideas of reactions, particularly when we consider that elementary reactions (only for which we can write rate expressions based on molecularity and order mapping) can be thought of proceeding due to collisions (or interactions of some sort) of monomers (unimolecular), dimers(bimolecular), trimers (trimolecular), etc. -
Empirical Chemical Kinetics
Empirical Chemical Kinetics time dependence of reactant and product concentrations e.g. for A + 2B → 3C + D d[A] 1 d[B] 1 d[C] d[D] rate =− =− = = d2d3ddtttt =ν In general, a chemical equation is 0∑ ii R i nt()− n (0 ) The extent of a reaction (the advancement) = ii ν i For an infinitesmal advancement dξ each reactant/product =ν ξ concentration changes by d[Ri ]i d . d1d[R]ξ By definition, the rate == i ν ddtti Reaction rates usually depend on reactant concentrations, e.g., rate= k [A]xy [B] order in B total order = x+y rate constant In elementary reaction steps the orders are always integral, but they may not be so in multi-step reactions. The molecularity is the number of molecules in a reaction step. Rate Laws d[A] Zero order: −=k dt 0 [A] = [A]00 -[A]t kt [A]0 t1 = 2 2k 0 0 t −=d[A] First order: k1[A] [A] ln[A] dt − = kt1 [A]t [A]0 e ln 2 0 t 0 t t1 = 2 k1 d[A] 2 Second order: −=2[A]k [A] dt 2 [A] [A] = 0 t + 12[A]kt20 0 t -1=+ -1 [A]t [A]02 2kt 1 t1 = 2 2[A]k20 [A]-1 0 t Second-order Kinetics: Two Reactants A + B k → products da rate=− =kab a = [A], b =[B] dt =− − ka()()00 x b x ddxa Since aa=− x, =− 0 ddtt dx So =−ka()() x b − x dt 00 x dx kt = ∫ ()()−− 0 axbx00 −111x =−dx ()−−−∫ ()() ab000 ax 0 bx 0 −1 ab = ln 0 ()− ab00 ab 0 or more usefully, aa=+−0 ln ln ()abkt00 bb0 Data Analysis “Classical” methods of data analysis are often useful to explore the order of reactions, or to display the results (e.g.