Chapter 14 Flashcards
(15 cards)
Describe the main factors that can increase the rate of reaction
Increase in temperature, increasing the concentration, and more surface area
Collision Theory
For a chemical reaction to occur the reacting particles must collide with one another
Effective collisions
result in the formation of a transition state or activated complex. Only effective collisions can result in product formation
Activation energy
Is the minimum energy that colliding molecules must possess in order for the collision to be effective
Reaction order
is the power to which the concentration of a given reactant is raised in the rate law equation. The overall reaction order is the sum of the powers to which reactant concentrations are raised in the rate law.
First order reaction
is proportional to the convention of a single reactant
Second order reactant
is proportional to the product of two reactants ([A][B]) or on the concentration of a single reactant squared ([A]^2 [B]^2)
The rate of a zeroth-order reaction
is a constant, independent of reactant concentration.
Reaction mechanism
is the series of individual steps by which an overall chemical reaction occurs.
Elementary reaction
is each step in a reaction mechanism
Catalyst
A substance that increases the rate of a chemical reaction without itself being consumed. It also speeds up a reactant usually by lowering the value of of the activation energy.
Intermediate
A chemical species that is produced in one step of a reaction mechanism and consumed in a following step.
Heterogeneous catalysis
A catalysis in which the reactants and the catalysis are in different places.
Homogeneous catalysis
A catalysis in which the reactants and the catalyst are in the same place
Enzymatic catalysis
is the increase in the rate of a process by an enzyme, a biological molecule.
