Chapter 14 Flashcards
(16 cards)
Chemical kinetics
the study of reaction rates, how reaction rates change under varying conditions, and what molecular events occur during the overall reaction
Factors affect reaction rates
1) physical state of reactants
2) reactant concentration
3) reaction temperature
4) pressure of a catalyst
Reaction rate
a positive quantity that expresses how the concentration of a reactant or product changes with time
Rate=
(delta [concentration])/ delta time
time and concentration dependent
k
the rate constant for the reaction
Rate law
rate= k[A][B]
Half life (t1/2)
the time required for the reactant concentration to decrease to one-half of its initial value
Collision theory
assumes that for a reaction to occur, reactant molecules must collide with the proper orientation and sufficient energy, meaning not very collision forms product
Ea
activation energy; the minimum energy of collision required for two molecules to react
Transition-state theory
the reaction resulting from the collision of two molecules in terms of an activated complex
Activated complex
an unstable grouping of atoms that can break up to form products
Transition state
the high point of a diagram
Molecularity
tells how many molecules are involve in the process
Reaction mechanism
the sequence of events that describes the actual process by which reactants become products
Catalysts
increase the rate of a reaction by decreasing the activation energy of the reaction
Enzymes
catalysts in biological systems
