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Related Concept Videos

Activation Energy01:26

Activation Energy

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Activation energy is the minimum amount of energy necessary for a chemical reaction to move forward. The higher the activation energy, the slower the rate of the reaction. However, adding heat to the reaction will increase the rate, since it causes molecules to move faster and increase the likelihood that molecules will collide. The collision and breaking of bonds represents the uphill phase of a reaction and generates the transition state. The transition state is an unstable high-energy state...
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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.
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A reversible chemical reaction represents a chemical process that proceeds in both forward (left to right) and reverse (right to left) directions. When the rates of the forward and reverse reactions are equal, the concentrations of the reactant and product species remain constant over time and the system is at equilibrium. A special double arrow is used to emphasize the reversible nature of the reaction. The relative concentrations of reactants and products in equilibrium systems vary greatly;...
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Thermal cycloadditions are reactions where the source of activation energy needed to initiate the reaction is provided in the form of heat. A typical example of a thermally-allowed cycloaddition is the Diels–Alder reaction, which is a [4 + 2] cycloaddition. In contrast, a [2 + 2] cycloaddition is thermally forbidden.
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Cycloaddition Reactions: MO Requirements for Photochemical Activation01:12

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Some cycloaddition reactions are activated by heat, while others are initiated by light. For example, a [2 + 2] cycloaddition between two ethylene molecules occurs only in the presence of light. It is photochemically allowed but thermally forbidden.
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Imine Metathesis by Silica-Supported Catalysts Using the Methodology of Surface Organometallic Chemistry
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Self-activated surface dynamics in gold catalysts under reaction environments.

Naoto Kamiuchi1, Keju Sun1,2,3, Ryotaro Aso1

  • 1The Institute of Scientific and Industrial Research, Osaka University, 8-1 Mihogaoka, Ibaraki, Osaka, 567-0047, Japan.

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This study reveals nanoporous gold (NPG) as a self-activating catalyst for CO oxidation. The key active sites are gold-silver oxide clusters, unifying understanding of gold catalyst mechanisms.

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Area of Science:

  • Materials Science
  • Catalysis
  • Surface Chemistry

Background:

  • Nanoporous gold (NPG) exhibits unique sponge-like structures.
  • Understanding the catalytic mechanisms of gold-based materials is crucial for developing efficient catalysts.

Purpose of the Study:

  • To investigate the surface dynamics and catalytic activity of NPG in the oxidation of carbon monoxide (CO) at room temperature.
  • To identify the fundamental active structure responsible for NPG's catalytic performance.

Main Methods:

  • Atomic-scale and microsecond-resolution environmental transmission electron microscopy (ETEM).
  • Ab initio energy calculations.
  • In-situ observation under CO oxidation reaction conditions.

Main Results:

  • Observed peculiar surface dynamics involving gold, oxygen, and residual silver on NPG {110} facets.
  • Identified Au-AgO surface clusters as the essential structure unit for catalytic activity.
  • Classified NPG as a novel self-activating catalyst, potentially acting as a nano-structured silver oxide catalyst or an inverse supported gold nanoparticulate (AuNP) catalyst.

Conclusions:

  • The catalytically active structure in both supported AuNP and NPG catalysts for low-temperature CO oxidation can be experimentally unified.
  • This finding represents a significant step towards elucidating the catalytic mechanisms of gold.