Chemical Kinetics Flashcards
Name the three things that need to occur in order for a reaction to be successful
There needs to be the necessary amount of activation energy to break the bonds
There must be collisions
The collision must be in the correct orientation
What’s kinetics?
The study of the rates at which chemical processes occur
The four factors that affect reaction rates
Physical State
Concentration
Temperature
Presence of a catalyst
How do you fine the average rate
average rate = (delta)[concentration] / (delta) time
instantaneous rate
the rate at any given moment in a reaction
the slope of a line tangent to the curve at any point
Rate laws
Rate = k [A]^m [B]^n
Define Instantaneous Rate
The instantaneous rate determined just after the reactions begins
(t = 0)
Define half-life
the time required for one-half of a reactant to react
Define Activation energy
the minimum amount of energy required for reaction
Define a reaction coordinate diagrams
a diagram that shows visually the energy changes throughout a process
Reaction Coordinate Diagram: Define Transition State
The high point on the diagram
Reaction Coordinate Diagrams: Activated Complex
The species present at the transition state
Define Reaction Mechanism
The sequence of events that describes the actual process by which reactants become products
Define Elementary reaction or elementary process
Reactions may occur all at once or through several discrete steps
What does a catalyst do to a reaction?
catalysts increase the rate of a reaction by decreasing the activation energy of the reaction
catalysts change the mechanism by which the process occurs
