Chemical Kinetics and Rate Equations

These flashcards cover key vocabulary terms relevant to chemical kinetics and reaction rate equations, aiding students in their preparation for exams.

Chemical Reaction Rate

The speed at which reactants are converted into products over time.

Rate Constant (k)

A constant that relates the rate of a reaction to the concentration of reactants.

Order of Reaction (n)

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

Zero Order Reaction

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

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 a reactant.

Half-Life (t1/2)

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

Concentration Units

Expressed typically in molarity (mol/L) for reactions.

Reaction Mechanism

The sequence of elementary steps that collectively represent the overall reaction.

Activation Energy (Ea)

The minimum energy required for a reaction to occur.

Arrhenius Equation

A formula that relates the rate constant to temperature and activation energy: k = A e^{-Ea/RT}.

Rate Law

An equation that relates the rate of a reaction to the concentration of reactants, e.g. r = k[A]^n.

Equilibrium Constant (K)

A value that expresses the ratio of products to reactants at equilibrium.

Catalyst

A substance that increases the rate of a reaction without being consumed in the process.