The speed at which a chemical reaction occurs.
Chemical reactions: Understanding of what a chemical reaction is and how it occurs is essential before delving into reaction rates.
Reaction rate: The study of how quickly or slowly a chemical reaction occurs and how the rate changes over time.
Factors affecting reaction rate: This includes the concentration of reactants, temperature, surface area, catalysts, and pressure which affect the rate of the reaction.
Rate law and rate constants: The mathematical relationship between the rate of a chemical reaction and the concentrations of its reactants and products.
Reaction mechanisms: The sequence of individual chemical steps that take place during a chemical reaction.
Activation energy and transition states: The minimum energy required to initiate a chemical reaction and the intermediate state between reactants and products.
Collisions theory: A theory that explains how chemical reactions occur by the collision of molecules with sufficient energy.
Arrhenius equation: An equation that relates the rate constant of a chemical reaction to the temperature at which it occurs.
Reaction order: A concept that describes the relationship between the rate of a chemical reaction and the concentration of reactants.
Half-life: The time taken for the concentration of a reactant to decrease by half.
Enzyme kinetics: The study of the rates at which enzymes catalyze chemical reactions.
Chemical equilibrium: The state of a chemical reaction where the forward and reverse reactions occur at equal rates.
Reaction kinetics in industry: Application of reaction kinetics in industrial processes including the design and optimization of chemical reactors.
Kinetics in atmospheric chemistry: Understanding the rates at which chemical reactions occur in the earth's atmosphere.
Kinetics in biological systems: The study of the rates of biochemical reactions that occur in living cells.
Zero-order reaction: This type of reaction rate is independent of the concentration of the reactants. The reaction proceeds at a constant rate.
First-order reaction: This type of reaction rate depends on the concentration of one of the reactants. The rate constant is proportional to the concentration of that reactant.
Second-order reaction: This type of reaction rate depends on the concentration of two reactants. The rate constant is proportional to the product of the concentrations of the two reactants.
Third-order reaction: This type of reaction rate depends on the concentration of three reactants. The rate constant is proportional to the product of the concentrations of the three reactants.
Pseudo-first-order reaction: This type of reaction rate is a first-order reaction in which one of the reactants is in such an excess that its concentration can be considered constant.
Enzymatic reaction: This type of reaction is catalyzed by enzymes. The rate of the reaction depends on the concentration of the enzyme and the substrate.
Photochemical reaction: This type of reaction is initiated by absorption of light. The reaction occurs when a molecule absorbs a photon and becomes excited.
Thermal reaction: This type of reaction occurs when molecules are exposed to heat. The energy of the heat causes the molecules to undergo a chemical transformation.
Radical reaction: This type of reaction is initiated by free radicals. The rate of the reaction depends on the concentration of the radicals.
Heterogeneous reaction: This type of reaction occurs at the interface between two phases, such as a solid and a gas or a liquid and a gas.
Homogeneous reaction: This type of reaction occurs within a single phase, such as a gas or a liquid.
Surface reaction: This type of reaction occurs at the surface of a solid. The reaction rate depends on the surface area of the solid.
Oscillatory reaction: This type of reaction exhibits periodic oscillations in the concentrations of the reactants and products.
Autocatalytic reaction: This type of reaction is catalyzed by one of the products of the reaction. The reaction rate increases as the concentration of the catalyst (one of the products) increases.
Inhibited reaction: This type of reaction is slowed down or stopped by the presence of an inhibitor. The rate of the reaction decreases as the concentration of the inhibitor increases.