Rates of Chemical Reactions

These flashcards cover key concepts and definitions related to the rates of chemical reactions, as discussed in the lecture notes.

Rate of Reaction

The change in concentration of a reactant or product with time.

Order of Reaction

The power to which the concentration of a reactant is raised in the rate law.

Rate Constant (k)

A proportionality constant in the rate equation, affected by temperature.

Zero Order Reaction

A reaction where the rate is constant and does not depend on the concentration of reactants.

First Order Reaction

A reaction where the rate is directly proportional to the concentration of one reactant.

Second Order Reaction

A reaction where the rate is proportional to the square of the concentration of one reactant.

Half-life of a Reaction

The time required for the concentration of a limiting reactant to decrease to half of its initial concentration.

Collision Theory

States that molecules must collide with sufficient energy and correct orientation to react.

Activation Energy (Ea)

The minimum energy required for reactants to collide and form products.

Catalyst

A substance that increases the rate of a chemical reaction without undergoing permanent change.

Maxwell-Boltzmann Distribution 

A curve that represents the distribution of kinetic energy among molecules in a sample.

Effective Collision

Collisions that result in a chemical reaction; requires sufficient energy and proper orientation.

Factors Affecting Reaction Rate

Temperature, concentration, surface area, catalyst presence, and pressure.

Monitoring Reaction Rates

Methods include measuring gas volume, loss of mass, color change, pH change, and electrical conductivity.