Swedish chemist Jöns Jacob Berzelius (1779-1848) analyzes earlier work on the role of sulfuric acid in promoting the conversion of ethanol to ether, shows that the hydrolysis of starch is catalyzed more efficiently by malt diastase than by sulphuric acid, and publishes the first general theory of chemical catalysis, introducing the terms "catalysis" (katalyska kraft), "catalyst" which he defined as "substances which by their mere presence evoke chemical reactions that would not otherwise take place." (He also coined the words "polymer", "isomer" and "allotrope", and named several chemical elements.)
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1877 |
German physiologist Wilhelm Kühne (1837-1900) introduces the word "enzyme" in connection with his discovery of trypsin. |
1907 |
German chemist Eduard Buchner (1860-1917) receives Nobel Prize in Chemistry for showing that juice squeezed out of yeast cells can ferment sugars — thus finally overturning the old vitalistic idea that biological reactions can only take place within living cells. |
1923 |
Almer McAffee develops the first commercially viable catalytic cracking process, doubling or tripling the yield of gasoline from crude oil.1937 |
1937 |
Eugene Houdree develops a catalytic cracking process that is able to change low-grade fuel oils into high-test gasoline |
1960 |
Planck and Rosinski develop the first zeoline catalyst for catalytic cracking |
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more cat history at http://www.nacatsoc.org/history.asp.
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What you should be able to do
Make sure you thoroughly understand the following essential ideas which have been presented above. It is especially imortant that you know the precise meanings of all the green-highlighted terms in the context of this topic.
- Describe the contrasting roles of thermodynamics and kinetics in understanding chemical change.
- Given a balanced net equation, write an expression for the rate of a reaction.
- Sketch a curve showing how the instantaneous rate of a reaction might change with time.
- Determine the order of a reaction of the form A → B + C from experimental data for the concentrations of its products at successive times.
- Describe the initial rate and isolation methods of determining the orders of the individual reactants in a reaction involving multiple reactants.
- Explain the difference between differential and integral rate laws.
- Sketch out a plot showing how the concentration of a component ([A] or ln [A]) that follows first-order kinetics will change with time. Indicate how the magnitude of the rate constant affects this plot
- Define the half-life of a reaction.
- Given the half-life for a first-order reaction A → products along with the initial value of [A]o, find [A]t at a subsequent time an integral number of half-lifes later.
- Describe the conditions under which a reaction can appear to have an order of zero.
Concept Map

