CHEM 102 Chapter Notes - Chapter 15: Collision Theory, Reaction Rate Constant, Stoichiometry
9 Mar 2016
School
Department
Course
Professor
Document Summary
Reaction rate: how fast or slow a reaction takes place. Definition of the rate of the reaction is written as . Reactants are always negative and the products are positive. The minimum quantity of energy that the reacting species must possess in order to undergo a specified reaction. Transition state: high-energy intermediate state to get reactants to the product. Definitio n: a substance that speeds up a chemical reaction, but is not consumed by the reaction; hence a catalyst can be recovered. How they work; also called enzymes are important in biology. A catalyst works by providing an alternative reaction pathway to the reaction product. The rate of the reaction is increased as this alternative route has a lower activation energy than the reaction route not mediated by the catalyst. Examples: chlorine in the decomposition of ozone. Catalytic converters: in a car help eliminate pollutants (that help form ozone) in the exhaust. Ozone is a pollutant in the lower atmosphere.
