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Lecture

Catalysis: History and Modern Challenges

In course

CH-422: Catalyst design for synthesis

This course on homogeneous catalysis provide a detailed understanding of how these catalysts work at a mechanistic level and give examples of catalyst design for important reactions (hydrogenation, olefin metathesis, cross-coupling). ...

Description

This lecture covers the history of catalysis, starting with Jons J. Berzelius' introduction of the concept in 1835. It explores the Nobel Prizes awarded for catalysis advancements, such as the Haber-Bosch process and modern polymerization catalysis. The lecture also delves into the types of catalysis, catalyst parameters, and the challenges faced in catalysis today, including renewable materials and energy domain applications.

Instructor

Xile Hu

Xile Hu was born in 1978 in Putian, southeastern China. He entered the Peking University in Beijing in 1996. Besides learning too little chemistry, his biggest regret in the college was not able to correct his southern accent in Mandarin. After graduated from PKU, he went to the United States and began his doctoral studies at the University of California, San Diego. In December 2004, he finished with a Ph.D. in chemistry and some fond memories of the beautiful city of San Diego. He then moved to the Los Angeles area and become a postdoctoral scholar at the California Institute of Technology. There he enjoyed numerous stimulating scientific (and other) discussions with friends and colleagues. He also made plenty of friends outside the campus and was a frequent in many local Chinese restaurants. In 2007, after two pleasant visits to Switzerland, he decided to move across the continent one more time and join the faculty of the École Polytechnique Fédérale de Lausanne (EPFL). He now directs the Laboratory of Inorganic Synthesis and Catalysis and is interested in developing chemistry for synthesis, energy and sustainability.

Official source

Related concepts (32)

Catalysis

Catalysis (kəˈtæləsɪs) is the process of change in rate of a chemical reaction by adding a substance known as a catalyst (ˈkætəlɪst). Catalysts are not consumed by the reaction and remain unchanged after it. If the reaction is rapid and the catalyst recycles quickly, very small amounts of catalyst often suffice; mixing, surface area, and temperature are important factors in reaction rate. Catalysts generally react with one or more reactants to form intermediates that subsequently give the final reaction product, in the process of regenerating the catalyst.

Homogeneous catalysis

In chemistry, homogeneous catalysis is catalysis where the catalyst is in same phase as reactants, principally by a soluble catalyst a in solution. In contrast, heterogeneous catalysis describes processes where the catalysts and substrate are in distinct phases, typically solid-gas, respectively. The term is used almost exclusively to describe solutions and implies catalysis by organometallic compounds. Homogeneous catalysis is an established technology that continues to evolve.

Heterogeneous catalysis

Heterogeneous catalysis is catalysis where the phase of catalysts differs from that of the reactants or products. The process contrasts with homogeneous catalysis where the reactants, products and catalyst exist in the same phase. Phase distinguishes between not only solid, liquid, and gas components, but also immiscible mixtures (e.g. oil and water), or anywhere an interface is present. Heterogeneous catalysis typically involves solid phase catalysts and gas phase reactants.

Chemical reaction

A chemical reaction is a process that leads to the chemical transformation of one set of chemical substances to another. Classically, chemical reactions encompass changes that only involve the positions of electrons in the forming and breaking of chemical bonds between atoms, with no change to the nuclei (no change to the elements present), and can often be described by a chemical equation. Nuclear chemistry is a sub-discipline of chemistry that involves the chemical reactions of unstable and radioactive elements where both electronic and nuclear changes can occur.

Reaction rate

The reaction rate or rate of reaction is the speed at which a chemical reaction takes place, defined as proportional to the increase in the concentration of a product per unit time and to the decrease in the concentration of a reactant per unit time. Reaction rates can vary dramatically. For example, the oxidative rusting of iron under Earth's atmosphere is a slow reaction that can take many years, but the combustion of cellulose in a fire is a reaction that takes place in fractions of a second.

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