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Related Concept Videos

Homogeneous Equilibria for Gaseous Reactions02:15

Homogeneous Equilibria for Gaseous Reactions

Homogeneous Equilibria for Gaseous Reactions
For gas-phase reactions, the equilibrium constant may be expressed in terms of either the molar concentrations (Kc) or partial pressures (Kp) of the reactants and products. A relation between these two K values may be simply derived from the ideal gas equation and the definition of molarity. According to the ideal gas equation:
Chemical Equilibria: Systematic Approach to Equilibrium Calculations01:21

Chemical Equilibria: Systematic Approach to Equilibrium Calculations

Equilibrium calculations for systems involving multiple equilibria are often complex. For example, to calculate the solubility of a sparingly soluble salt in an aqueous solution in the presence of a common ion, one must consider all the equilibria in this solution. Calculations for these systems can be complicated and tedious, so a systematic approach with a series of steps is often helpful. The process is detailed below.
The first step is to identify all the chemical reactions involved, The...
Calculating the Equilibrium Constant02:46

Calculating the Equilibrium Constant

The equilibrium constant for a reaction is calculated from the equilibrium concentrations (or pressures) of its reactants and products. If these concentrations are known, the calculation simply involves their substitution into the Kc expression.
For example, gaseous nitrogen dioxide forms dinitrogen tetroxide according to this equation:
Chemical Stoichiometry and Gases: Using Ideal Gas Law to Determine Moles03:12

Chemical Stoichiometry and Gases: Using Ideal Gas Law to Determine Moles

Chemical stoichiometry describes the quantitative relationships between reactants and products in chemical reactions.
Multi-Step Reactions02:31

Multi-Step Reactions

Chemical reactions often occur in a stepwise fashion involving two or more distinct reactions taking place in a sequence. A balanced equation indicates the reacting species and the product species, but it reveals no details about how the reaction occurs at the molecular level. The reaction mechanism (or reaction path) provides details regarding the precise, step-by-step process by which a reaction occurs. Each of the steps in a reaction mechanism is called an elementary reaction. These...
Calculating Equilibrium Concentrations02:05

Calculating Equilibrium Concentrations

Being able to calculate equilibrium concentrations is essential to many areas of science and technology—for example, in the formulation and dosing of pharmaceutical products. After a drug is ingested or injected, it is typically involved in several chemical equilibria that affect its ultimate concentration in the body system of interest. Knowledge of the quantitative aspects of these equilibria is required to compute a dosage amount that will solicit the desired therapeutic effect.
A more...

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Related Experiment Video

Updated: Jul 20, 2026

Combustion Chemistry of Fuels: Quantitative Speciation Data Obtained from an Atmospheric High-temperature Flow Reactor with Coupled Molecular-beam Mass Spectrometer
07:24

Combustion Chemistry of Fuels: Quantitative Speciation Data Obtained from an Atmospheric High-temperature Flow Reactor with Coupled Molecular-beam Mass Spectrometer

Published on: February 19, 2018

Master equation methods in gas phase chemical kinetics.

James A Miller1, Stephen J Klippenstein

  • 1Combustion Research Facility, Sandia National Laboratories, Livermore, CA 94551-0969, USA. jamille@sandia.gov

The Journal of Physical Chemistry. A
|September 8, 2006
PubMed
Summary

Master equation methods are applied to complex gas phase chemical kinetics, focusing on multi-well reactions and radical dissociation crucial for combustion chemistry.

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Area of Science:

  • Chemical Kinetics
  • Combustion Chemistry

Background:

  • Complex reaction pathways involving multiple potential wells are common in gas phase chemistry.
  • The dissociation of weakly bound free radicals is a critical process in combustion.

Purpose of the Study:

  • To discuss the application of master equation methods to gas phase chemical kinetics.
  • To highlight the importance of these methods for understanding multi-well reactions and radical dissociation.
  • To provide examples from previously studied reactions.

Main Methods:

  • Application of master equation methods.
  • Analysis of reactions over interconnected potential wells.
  • Study of dissociation dynamics of weakly bound free radicals.

Main Results:

  • Demonstration of master equation methods' utility in complex chemical kinetics.
  • Insights into reaction mechanisms in combustion chemistry.
  • Illustrative examples of specific reaction dynamics.

Conclusions:

  • Master equation methods are effective tools for studying complex gas phase reactions.
  • These methods are vital for advancing the understanding of combustion chemistry.
  • The presented examples showcase the practical application and insights gained.