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Principle of Least Time in Chemical Kinetics
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B. A. Mosienko
Veröffentlicht/Copyright:
22. September 2010
Abstract
The analogy between the principle of least time in optics (Fermat’s principle) and Ostwald’s rule of intermediate steps made it possible to set up the principle of least time for first-order phase transitions. In its turn, the analogy between first-order phase transitions and chemical reactions allows assume that the principle of least time is also valid in chemical kinetics. This assumption is substantiated in the given work. Also proposed is a different derivation of the indicated principle based on generalization of empirical data.
Keywords: Fermat’s Principle in Optics; Ostwald’s Rule of Intermediate Steps; Phase Transitions of First Kind; Intermediate stages; Chemical Reactions
Published Online: 2010-9-22
Published in Print: 2010-9-1
© by Oldenbourg Wissenschaftsverlag, Novosibirsk, Germany
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- Mass Transfer to Microelectrodes and Arrays
- Fluorescence Quenching of Phycoerythrin by Anthraquinone Dyes
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- Crystal Structure and Solid–Solid Phase Transition of 1-Dodecylamine Hydrobromide
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Schlagwörter für diesen Artikel
Fermat’s Principle in Optics;
Ostwald’s Rule of Intermediate Steps;
Phase Transitions of First Kind;
Intermediate stages;
Chemical Reactions
Artikel in diesem Heft
- Synthesis, Characterization and CMC Determination of some Double-Chain Surfactant-Cobalt(III) Complexes
- Mass Transfer to Microelectrodes and Arrays
- Fluorescence Quenching of Phycoerythrin by Anthraquinone Dyes
- Principle of Least Time in Chemical Kinetics
- Synthesis and Viscoelastic Behavior of an Anionic Gemini Surfactant in Aqueous Solution
- Hydrophobic Nature of the Support: a Significant Effect on Selective Oxidation of Cyclohexane with Pure Oxygen
- Crystal Structure and Solid–Solid Phase Transition of 1-Dodecylamine Hydrobromide
- Comparative Study of the Absolute Values of Enthalpy and Gibbs Free Energy of Solvation of Proton from Cluster-ion Solvation data and Direct Determination of the Thermodynamic Parameters of Proton in Aqueous and Non-aqueous Solvents
