Transition state theory
In chemistry, transition state theory (TST) explains the reaction rates of elementary chemical reactions. The theory assumes a special type of chemical equilibrium (quasi-equilibrium) between reactants and activated transition state complexes. This theory was developed simultaneously in 1935 by Henry Eyring, then at Princeton University, and by Meredith Gwynne Evans and Michael Polanyi of the University of Manchester. TST is also referred to as "activated-complex theory", "absolute-rate theory", and "theory of absolute reaction rates".
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- enIn chemistry, transition state theory (TST) explains the reaction rates of elementary chemical reactions. The theory assumes a special type of chemical equilibrium (quasi-equilibrium) between reactants and activated transition state complexes. This theory was developed simultaneously in 1935 by Henry Eyring, then at Princeton University, and by Meredith Gwynne Evans and Michael Polanyi of the University of Manchester. TST is also referred to as "activated-complex theory", "absolute-rate theory", and "theory of absolute reaction rates".
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- enApril 2015
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- enIn chemistry, transition state theory (TST) explains the reaction rates of elementary chemical reactions. The theory assumes a special type of chemical equilibrium (quasi-equilibrium) between reactants and activated transition state complexes. TST is used primarily to understand qualitatively how chemical reactions take place. TST has been less successful in its original goal of calculating absolute reaction rate constants because the calculation of absolute reaction rates requires precise knowledge of potential energy surfaces, but it has been successful in calculating the standard enthalpy of activation (ΔH‡, also written Δ‡Hɵ), the standard entropy of activation (ΔS‡ or Δ‡Sɵ), and the standard Gibbs energy of activation (ΔG‡ or Δ‡Gɵ) for a particular reaction if its rate constant has been experimentally determined. (The ‡ notation refers to the value of interest at the transition state; ΔH‡ is the difference between the enthalpy of the transition state and that of the reactants.) This theory was developed simultaneously in 1935 by Henry Eyring, then at Princeton University, and by Meredith Gwynne Evans and Michael Polanyi of the University of Manchester. TST is also referred to as "activated-complex theory", "absolute-rate theory", and "theory of absolute reaction rates". Before the development of TST, the Arrhenius rate law was widely used to determine energies for the reaction barrier. The Arrhenius equation derives from empirical observations and ignores any mechanistic considerations, such as whether one or more reactive intermediates are involved in the conversion of a reactant to a product. Therefore, further development was necessary to understand the two parameters associated with this law, the pre-exponential factor (A) and the activation energy (Ea). TST, which led to the Eyring equation, successfully addresses these two issues; however, 46 years elapsed between the publication of the Arrhenius rate law, in 1889, and the Eyring equation derived from TST, in 1935. During that period, many scientists and researchers contributed significantly to the development of the theory.
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- Age of the universe
- Arrhenius equation
- Boltzmann constant
- Category:Chemical kinetics
- Category:Chemistry theories
- Chemical activity
- Chemical equilibrium
- Chemical reaction
- Chemistry
- Classical mechanics
- Collision theory
- Curtin–Hammett principle
- Dennis A. Dougherty
- Enthalpy
- Entropy of activation
- Enzyme catalysis
- Equilibrium constant
- Eugene Wigner
- Eyring equation
- File:Quasi-equilibrium1.jpg
- File:Rxn coordinate diagram 5.PNG
- Gibbs energy
- Hans Kramers
- Henry Eyring (chemist)
- Jacobus van 't Hoff
- James Clerk Maxwell
- Karl Ferdinand Herzfeld
- Kinetic theory of gases
- Leopold Pfaundler
- Linus Pauling
- Ludwig Boltzmann
- Max Trautz
- Maxwell–Boltzmann distribution
- Meredith Gwynne Evans
- Michael Polanyi
- Nonadiabatic transition state theory
- Phase space
- Physical organic chemistry
- Planck constant
- Potential energy surface
- Princeton University
- Reaction rate
- Reactive intermediate
- Reactivity-selectivity principle
- Reagent
- René Marcelin
- Richard Chace Tolman
- Ring flip
- Saddle point
- Semiclassical transition state theory
- Standard state
- Statistical mechanics
- Svante Arrhenius
- Thermodynamic temperature
- Thermodynamic versus kinetic reaction control
- Transition state
- Universal gas constant
- University of Manchester
- University of North Carolina at Chapel Hill
- Van 't Hoff equation
- Variational transition-state theory
- Vibrational frequency
- William Lewis (chemist)
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- Siirtymätilateoria
- Teoria de l'estat de transició
- Teoría del estado de transición
- Teoria dello stato di transizione
- Théorie de l'état de transition
- Theorie des Übergangszustandes
- Transition state theory
- Trantsizio egoeraren teoria
- نظرية تحول الحالة
- نظریه حالت گذار
- 过渡态理论
- 遷移状態理論
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- Category:Chemical kinetics
- Category:Chemistry theories
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