Kinetics

These flashcards cover key vocabulary and concepts related to the topic of Kinetics from the lecture notes.

Kinetics

The study of chemical reaction rates.

Rate Expression

A mathematical representation of the rate of a reaction.

Molarity

The concentration of a solution expressed in moles of solute per liter of solution.

Collision Theory

A theory stating that reactants must collide to react with each other.

Activation Energy (Ea)

The minimum energy required for a reaction to occur.

Catalyst

A substance that increases the rate of a chemical reaction by lowering the activation energy without being consumed.

Reaction Rate

The speed at which a chemical reaction proceeds, typically measured by the change in concentration of reactants or products over time.

Instantaneous Reaction Rate

The rate of a reaction at a specific time, calculated using a graph of concentration versus time.

Average Reaction Rate

The rate of a reaction measured over a specific time period.

Integrated Rate Law

An equation that relates the concentration of a reactant to time, depending on the reaction order.

First-Order Reaction

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

Rate Law

An equation that relates the rate of a reaction to the concentration of reactants.

Zero Order Reaction

A reaction where the rate is independent of the concentration of the reactant.

Second-Order Reaction

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

Half-Life

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

Effective Collision

A collision between reactants that leads to a chemical reaction.

Heterogeneous Catalyst

A catalyst that is in a different phase from the reactants.

Homogeneous Catalyst

A catalyst that is in the same phase as the reactants.

Enzyme

A biocatalyst, typically a protein, that catalyzes biological reactions.

Reaction Coordinate

A graphical representation showing the progress of a reaction from reactants to products.

Stoichiometric Factors

Coefficients in a balanced chemical equation used to relate the rates of reactants and products.