Kinetics and Equilibrium Lecture Review

These flashcards cover key vocabulary terms related to kinetics and equilibrium in chemistry, providing definitions and explanations for better understanding of the concepts.

Kinetics

The study of the rate of change in concentrations of reactants and products in a chemical reaction.

Collision Theory

States that a reaction is most likely to occur if reactant particles collide with sufficient energy and proper orientation.

Catalyst

A substance that increases the rate of a reaction by providing an alternate pathway with lower activation energy, remaining unchanged in the process.

Activation Energy

The minimum energy required for a reaction to occur.

Exothermic Reaction

A reaction that releases energy; results in a negative change in enthalpy (∆H).

Endothermic Reaction

A reaction that absorbs energy; results in a positive change in enthalpy (∆H).

Potential Energy Diagram

A graph that shows the amount of energy absorbed or released during a chemical reaction as a function of the reaction coordinate.

Entropy

A measure of randomness or disorder in a system; reactions tend to occur towards higher entropy.

Gibbs Free Energy (∆G)

A criterion for spontaneity of a reaction; reactions are spontaneous if the value is negative.

LeChatelier’s Principle

States that if a system at equilibrium is subjected to a stress, the equilibrium will shift to counteract the stress.