Chemical kinetics

Chemical kinetics studies how fast chemical reactions occur, how conditions affect their rates, and the sequences of molecular steps by which they proceed.

Rate law: An equation relating a reaction rate to reactant concentrations, usually with experimentally determined exponents. Its concentration dependence summarizes the kinetic behavior measured for a reaction.
Reaction rate: The change in reactant or product concentration per unit time during a chemical reaction. Chemical kinetics explains how this observable quantity changes with conditions.
Catalysis: The acceleration of a chemical reaction by a substance that is regenerated during the process. Catalysts change reaction pathways and lower kinetic barriers without changing equilibrium.
Chemical equilibrium: A state in which forward and reverse reaction rates are equal, leaving macroscopic composition constant. Equilibrium specifies the final balance, not how quickly it is reached.
Ludwig Wilhelmy: A German chemist who used polarimetry to quantify the rate of acid-catalyzed sucrose inversion in 1850. His work is often cited as an early quantitative study of reaction rates.
Reaction mechanism: A sequence of elementary molecular steps that produces the overall chemical reaction. Kinetic evidence helps distinguish proposed sequences of elementary steps.
Rate constant: A proportionality constant in a rate law whose value depends on temperature and other conditions. It separates a reaction’s characteristic speed from its concentration dependence.
Enzyme kinetics: The study of reaction rates catalyzed by enzymes and their dependence on substrate and inhibitor concentrations. It applies kinetic principles to biological catalysts and their regulation.
Chemical thermodynamics: The study of energy, entropy, and equilibrium constraints in chemical systems. Thermodynamics predicts favorability, while kinetics determines rates and pathways.
Svante Arrhenius: A Swedish physical chemist who formulated the temperature-dependent Arrhenius equation. His equation remains a basic tool for interpreting temperature effects on rates.

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