Biological Chemistry - Reaction Kinetics

These flashcards cover key vocabulary terms and definitions from the lecture on Reaction Kinetics.

Kinetics

The study of the speed or rate at which chemical reactions proceed.

Rate of reaction

The rate of change of concentration of reactants and products.

Reaction mechanism

A detailed step-by-step description of a chemical reaction, developed as a hypothesis to account for observed facts.

Energy of activation (Eact)

The minimum amount of energy required for particles to collide effectively and initiate a chemical reaction.

Exothermic reaction

A reaction in which heat is generated and released.

Endothermic reaction

A reaction that absorbs heat.

Activated complex

A very unstable intermediate state that occurs during the transition between reactants and products.

Catalyst

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

Law of mass action

At constant temperature, the rate of a reaction is proportional to the active masses of the reactants.

Arrhenius equation

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

Molecularity

The number of reactant molecules involved in the rate-determining step of a reaction.

Half-life (t1/2)

The time taken for 50% of the reactant to be consumed in a reaction.

First order reaction

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

Zero order reaction

A reaction where the rate is constant and does not change with concentration.

Order of reaction

An expression that relates to how the rate of reaction depends on the concentration of the reactants.

Chain reaction

A reaction that continues indefinitely once started, involving a series of steps regenerating reactive radicals.