Temperature, Mechanisms and Catalysis

These flashcards cover key vocabulary terms related to temperature, mechanisms, and catalysis in chemistry, providing definitions for crucial concepts discussed in the lecture.

Collision Theory

A theory that describes how molecules collide in order for chemical reactions to occur.

Activation Energy (Ea)

The minimum energy that molecules must possess for a chemical reaction to occur.

Transition State Theory

A theory that explains the states or forms a system passes through during a reaction, particularly the activated complex.

Arrhenius Equation

An equation that shows how the rate constant (k) of a reaction depends on temperature and activation energy (Ea), expressed as k = Ae^(-Ea/RT).

Elementary Process

A step in a reaction mechanism where one or more reactants undergo a single molecular event, characterized by its rate law.

Multistep Reactions

Reactions that proceed through multiple elementary processes, where the rate is determined by the slowest step known as the rate-determining step.

Catalysis

The process of accelerating a chemical reaction by the addition of a catalyst that is not consumed in the reaction.

Homogeneous Catalysis

Catalysis that occurs when all reactants, products, and catalysts are in the same phase, usually in solution.

Heterogeneous Catalysis

Catalysis that occurs when the catalyst is in a different phase, typically solid, while reactants and products may be in liquid or gas.

Kinetic-Molecular Theory (KMT)

A theory that explains the behavior of gases in terms of particle motion and interactions.