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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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The Collision Theory
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SN2 substitutions and E2 eliminations of alkyl halides proceed via a concerted pathway. While the nucleophile attacks the alpha carbon in SN2 reactions, it functions as a strong base and abstracts a beta hydrogen in the E2 mechanism. The rate-limiting transition state in E2 elimination reactions is characterized by partially broken carbon–hydrogen and carbon–halogen bonds and a partially formed pi bond between the alpha and beta carbons. The beta hydrogen and halide are eliminated...
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Here, in contrast to the E2 reaction mechanism, we delve into the aspects of the E1 reaction mechanism, which has two steps: rate-limiting loss of the leaving group and abstraction of the beta hydrogen by a weak base. Typically, the experimental proof for the E1 mechanism is via kinetic studies or isotope studies. While the former demonstrates the first-order kinetics—the dependence of the reaction solely on substrate concentration—the latter proves the abstraction of hydrogen only...
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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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Anisotropic Reaction Kinetics of Oxygen With Pyrolytic Graphite.

William S Horton1

  • 1Institute for Materials Research, National Bureau of Standards, Washington, D.C. 20234.

Journal of Research of the National Bureau of Standards. Section A, Physics and Chemistry
|June 12, 2020
PubMed
Summary
This summary is machine-generated.

Pyrolytic graphite

Keywords:
Chemical anisotropychemisorptionoxidationpyrolytic graphite

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Area of Science:

  • Materials Science
  • Chemical Engineering
  • Aerospace Engineering

Background:

  • Pyrolytic graphite's reaction with oxygen is crucial for aerospace applications.
  • Previous studies show conflicting results on graphite's chemical anisotropy and temperature dependence.
  • Discrepancies may stem from variations in sample type (single crystal vs. pyrolytic) and oxidizers used.

Purpose of the Study:

  • To investigate the chemical anisotropy of pyrolytic graphite's reaction with oxygen-containing gases.
  • To clarify the temperature dependence of pyrolytic graphite oxidation rates.
  • To determine the activation energies for key reaction steps.

Main Methods:

  • Oxidation of pyrolytic graphite samples with varying geometries in oxygen-containing gases.
  • Analysis of reaction rate differences between different crystallographic directions.
  • Application of kinetic models to determine rate-controlling steps and activation energies.

Main Results:

  • The rate ratio of pyrolytic graphite oxidation along different directions is temperature-dependent.
  • An activation energy difference of approximately 19 kJ/mol exists between the two major directions.
  • Chemisorption is rate-controlling on "faces," while decomposition is rate-controlling on "edges."

Conclusions:

  • The observed rate differences are attributed to varying site availability and shifts in rate-controlling steps.
  • Activation energy for chemisorption on "faces" is 131 kJ/mol.
  • Activation energy for decomposition on "edges" is 150 kJ/mol.