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Related Concept Videos

Reaction Rate02:53

Reaction Rate

The rate of reaction is the change in the amount of a reactant or product per unit time. Reaction rates are therefore determined by measuring the time dependence of some property that can be related to reactant or product amounts. Rates of reactions that consume or produce gaseous substances, for example, are conveniently determined by measuring changes in volume or pressure.
The mathematical representation of the change in the concentration of reactants and products, over time, is the rate...
Reaction Mechanisms: Rate-limiting Step Approximation01:29

Reaction Mechanisms: Rate-limiting Step Approximation

The rate-determining step, or RDS, in a chemical reaction is the slowest step that determines the overall reaction rate. It is identified by using the observed rate law and typically involves approximation methods like the RDS approximation or the steady-state approximation.In the RDS approximation, also known as the rate-limiting-step or equilibrium approximation, the reaction mechanism consists of one or more reversible reactions near equilibrium, followed by a slower RDS, and then one or...
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...
Heterogeneous Catalysis01:22

Heterogeneous Catalysis

Heterogeneous catalysis involves a catalyst in a different phase from the reactants. It is a process where the catalyst and the reactants are in distinct phases, typically solid and gas or liquid.Most heterogeneous catalysts are metals, metal oxides, or acids. The list includes transition metals like iron (Fe), cobalt (Co), nickel (Ni), palladium (Pd), platinum (Pt), chromium (Cr), manganese (Mn), tungsten (W), silver (Ag), and copper (Cu). These metals possess partially vacant d orbitals that...
Theories of Dissolution: Diffusion Layer Model01:15

Theories of Dissolution: Diffusion Layer Model

Dissolution, the process by which drug particles dissolve in a solvent, is explained by the diffusion layer model, a theoretical framework that simulates the absorption of oral drugs and allows us to analyze experimental data.
This process starts with a thin layer, saturated with the drug, forming at the interface between the solid and liquid. The solute then diffuses from this layer into the main solution. The Noyes-Whitney equation suggests that the rate of dissolution relies on the diffusion...
Measuring Reaction Rates03:09

Measuring Reaction Rates

Polarimetry finds application in chemical kinetics to measure the concentration and reaction kinetics of optically active substances during a chemical reaction. Optically active substances have the capability of rotating the plane of polarization of linearly polarized light passing through them—a feature called optical rotation. Optical activity is attributed to the molecular structure of substances. Normal monochromatic light is unpolarized and possesses oscillations of the electrical field in...

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Unraveling Entropic Rate Acceleration Induced by Solvent Dynamics in Membrane Enzymes
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Reaction rate calculations for cosubstrates diffusing into catalyst layer from opposite sides.

S F Karel1, C R Robertson

  • 1Department of Chemical Engineering, Stanford University, Stanford, California 94305, USA.

Biotechnology and Bioengineering
|August 20, 1987
PubMed
Summary
This summary is machine-generated.

This study examines diffusion effects in permeable catalysts with two substrates. Zeroth-order kinetics offer a reliable method for estimating reaction rates and positions within the catalyst layer.

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Area of Science:

  • Chemical Engineering
  • Catalysis Science
  • Reaction Engineering

Background:

  • Diffusion significantly impacts reactions within permeable catalysts.
  • Understanding substrate transport is crucial for catalyst design.
  • Multi-substrate reactions introduce complexities in predicting performance.

Purpose of the Study:

  • To theoretically analyze diffusion effects on reactions in permeable catalysts.
  • To investigate the influence of zeroth- and first-order kinetics on reaction-diffusion processes.
  • To develop a generalized method for estimating reaction rates and positions.

Main Methods:

  • Solving the reaction-diffusion equation for a catalytic slab geometry.
  • Analyzing solutions for combinations of zeroth- and first-order kinetics.
  • Defining effectiveness factors and reaction position parameters.

Main Results:

  • Reaction-diffusion solutions were obtained for various kinetic orders.
  • Results showed weak dependence of effectiveness factor on reaction order.
  • A parameter was identified to describe the location of the reaction zone.

Conclusions:

  • Zeroth-order kinetics provide a robust model for reaction-diffusion in this system.
  • The proposed method simplifies the estimation of reaction rates and positions.
  • This research offers insights into optimizing permeable catalyst performance.