Chapter 18 - Reaction rates of Equilibrium Flashcards
rate
is a measure of speed of any change that occurs within an interval of time
collision theory
atom, ect. can react to form products when they collide
activation theory
the minimum energy needed so colliding particles can react.
activated complex
an unstable arrangement of atoms that form momentarily at the peak of the activation-energy barrier (also known as the transition state )
inhibitor
a substance that breaks the catalyst
reversible reaction
when the conversion of reactants to products and the other way around, happen at the same time
chemical equilibrium
when the rates forward and backward are equal
Le Chátelier’s principle
If stress is applied to a system in equilibrium, the system changes to relieve the stress
equilibrium constant
Keq={C}^c x{D}^d / {A}^a x {B}^b
common ion
an ion that is found in both salts of a solution
free energy
energy that is ready to work
spontaneous reaction
occur naturally and favor the formation of products at specific conditions
nonspontaneous reaction
do not occur naturally and does not favor the formation of products at specific conditions
entropy
the measure of disorder
law of disorder
the lowest possible energy for a system
Gibbs free-energy change
the maximum amount of energy that can be doubled to another process to so useful work
rate law
the rate of reaction in terms of the concentration of the reactants
specific rate constant
(k) if k is large, the products form quickly; small they form slowly
first order reaction
the reaction rate is directly proportional to the concentration of one reactant
elementary reaction
reactants are converted to products in a single step
reaction mechanism
the series of steps that occur in a elementary reaction
intermediate
the product of one of the steps in the reaction mechanism
