Chemical Kinetics Flashcards
Gibbs free energy
determines whether or not a reaction will occur by itself without outside assistance
collision theory of chemical kinetics
the rate of a reaction is proportional to the number of collisions per second between the reacting molecules
chemical reaction rate
rate=Z+f
Z=total number of collisions occurring per second
f= fraction of collisions that are effective
frequency factor aka attempt frequency
measure of how often molecules in a certain reaction collide
reaction coordinate
traces the reaction from reactants to products
transition state aka activated complex
has greater energy than both the reactants and the products
free energy change of the reaction
difference between the free energy of the products and free energy of the reactants
homogenous catalysts
the catalyst is in the same phase as the reactants
heterogenous catalysts
the catalyst is in a different phase from the reactants
zero-order reaction
product C is independent of changes in concentration of any of the reactants, A and B
first-order reaction
rate that is directly proportional to only one reactant
second-order reaction
rate that is proportional to either the concentration of two reactants or to the square of the concentration of a single reactant
mixed-order reactions
refer to non-integer orders; also to reactions with rate orders that vary over the course of the reaction
broken-order
non-integer orders
