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Catalysis02:50

Catalysis

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A variety of factors influence the rate of chemical reactions. For a chemical reaction to happen, atoms must collide with enough energy to overcome the repulsion between their electrons. This energy is called activation energy. Factors influencing the rate of reaction either lower the activation energy or increase the likelihood of a successful collision.
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The Arrhenius equation relates the activation energy and the rate constant, k, for chemical reactions. In the Arrhenius equation, k = Ae−Ea/RT, R is the ideal gas constant, which has a value of 8.314 J/mol·K, T is the temperature on the kelvin scale, Ea is the activation energy in J/mole, e is the constant 2.7183, and A is a constant called the frequency factor, which is related to the frequency of collisions and the orientation of the reacting molecules.
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Kinetics describes the rate and path by which a reaction occurs. In contrast, thermodynamics deals with state functions and describes the properties, behavior, and components of a system. It is not concerned with the path taken by the process and cannot address the rate at which a reaction occurs. Although it does provide information about what can happen during a reaction process, it does not describe the detailed steps of what appears on an atomic or a molecular level. On the other hand,...
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Unraveling Entropic Rate Acceleration Induced by Solvent Dynamics in Membrane Enzymes
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Three-Factor Kinetic Equation of Catalyst Deactivation.

Zoë Gromotka1, Gregory Yablonsky2, Nickolay Ostrovskii3

  • 1Department of Electronics and Information Systems, Ghent University, 9000 Ghent, Belgium.

Entropy (Basel, Switzerland)
|July 2, 2021
PubMed
Summary

A new kinetic equation models catalyst deactivation, separating main reactions from reversible and irreversible aging processes. This approach accurately describes real-world catalyst behavior in chemical reactions.

Keywords:
catalyst deactivationkinetic equationreversible deactivation and agingseparability

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Area of Science:

  • Chemical kinetics
  • Catalysis science
  • Reaction engineering

Background:

  • Catalyst deactivation significantly impacts industrial process efficiency and economics.
  • Existing models often struggle to distinctly capture reversible and irreversible deactivation pathways.
  • Understanding these mechanisms is crucial for designing robust catalytic systems.

Purpose of the Study:

  • To develop a comprehensive kinetic equation for catalyst deactivation.
  • To differentiate and model the main catalytic cycle, reversible deactivation, and irreversible aging.
  • To validate the proposed model using literature data.

Main Methods:

  • Formulation of a three-factor kinetic equation based on apparent kinetic parameters.
  • Application of quasi-steady-state assumption for the main catalytic cycle.
  • Hierarchical separation of reversible and irreversible deactivation phenomena.
  • Mathematical analysis to determine conditions for separability.

Main Results:

  • A novel three-factor kinetic equation for catalyst deactivation was derived.
  • The equation successfully separates the main reaction cycle from reversible and irreversible deactivation.
  • The model accurately describes literature data for acetaldehyde dehydration and crotonaldehyde hydrogenation.

Conclusions:

  • The proposed kinetic equation provides a robust framework for understanding catalyst deactivation.
  • The hierarchical separation approach enhances the predictive power of kinetic models.
  • This work offers valuable insights for optimizing catalyst performance and longevity.