"The rate law or rate equation is an empirical mathematical expression for the rate of reaction of a particular reaction in terms of concentrations of chemical species and constant parameters."
An equation that describes the relationship between the rate of a chemical reaction and the concentration of its reactants.
Reaction rate: The speed at which a reaction occurs.
Stoichiometry: The relationship between reactants and products in a chemical reaction.
Concentration: The amount of a substance per unit volume.
Reaction order: The dependence of the rate on the concentration of reactants.
Rate constant: The proportionality constant in the rate law equation.
Integrated rate laws: Equations that relate concentration to time for different order reactions.
Half-life: The time it takes for half of the reactants to be converted into products.
Temperature dependence: The effect of temperature on the rate constant and overall reaction rate.
Activation energy: The energy required to initiate a reaction.
Catalysts: Substances that increase the reaction rate without being consumed in the reaction.
Rate-determining step: The slowest step in a multi-step reaction that determines the overall rate.
Arrhenius equation: A formula that relates the rate constant to temperature and activation energy.
Reaction mechanisms: A detailed description of the steps involved in a reaction.
Collision theory: A model that explains how reactions occur based on the collision of particles.
Enzyme kinetics: The study of rate laws for enzyme-catalyzed reactions.
Zero-order kinetics: The rate of the reaction is independent of the concentration of the reactants.
First-order kinetics: The rate of the reaction is directly proportional to the concentration of one of the reactants.
Second-order kinetics: The rate of the reaction is directly proportional to the product of the concentrations of two reactants, or the square of the concentration of one reactant.
Pseudo-first order kinetics: A second-order reaction that appears to be first-order due to the extremely high concentration of one reactant.
Enzyme kinetics: The rate of reaction involving enzymes, where the reaction rate depends on the substrate concentration, enzyme concentration, and reaction conditions.
Michaelis-Menten kinetics: A special type of enzyme kinetics that describes the relationship between substrate concentration and reaction rate.
Langmuir-Hinshelwood kinetics: A type of reaction kinetics that describes heterogeneous catalysis.
Eley-Rideal kinetics: A type of reaction kinetics that occurs on a surface, where one molecule or atom from the gas reacts with a molecule that is already bound to the surface.
Marcus theory: A type of electron transfer reaction kinetics, where the rate of electron transfer depends on the energy difference between the reactants and products.
Autocatalysis kinetics: A type of reaction kinetics where the reaction products themselves enhance the rate of reaction.
"The rate equation includes concentrations of chemical species and constant parameters, such as rate coefficients and partial orders of reaction."
"For many reactions, the initial rate is given by a power law expression."
"The initial rate is expressed as v0 = k[A]^x[B]^y, where [A] and [B] represent the concentrations of specific species."
"The exponents x and y are the partial orders of reaction for species A and B, respectively."
"The overall reaction order is the sum of the exponents, which quantifies the degree to which the rate of a chemical reaction depends on the concentrations of the reactants."
"Yes, the partial orders of reaction can be zero, fractional, or negative, in addition to positive integers."
"The reaction rate constant or rate coefficient, denoted as k, is a constant factor in the rate equation that determines the rate of the reaction."
"The value of the reaction rate constant may depend on conditions such as temperature, ionic strength, surface area of an adsorbent, or light irradiation."
"If the reaction goes to completion, the rate equation v = k[A]^x[B]^y applies throughout the course of the reaction."
"Yes, in elementary (single-step) reactions and reaction steps, the reaction orders are equal to the stoichiometric coefficients for each reactant."
"Yes, the overall reaction order is always equal to the molecularity of the elementary reaction."
"Complex (multi-step) reactions may or may not have reaction orders equal to their stoichiometric coefficients."
"No, the order and rate equation of a given reaction cannot be reliably deduced from the stoichiometry and must be determined experimentally."
"The rate equation of a reaction with an assumed multi-step mechanism can be derived theoretically using quasi-steady state assumptions and compared with the experimental rate equation as a test of the assumed mechanism."
"Yes, the rate equation may involve a fractional order and depend on the concentration of an intermediate species."
"Yes, a reaction can have an undefined reaction order if the rate is not simply proportional to some power of the concentration of that reactant."
"One example is a bimolecular reaction between adsorbed molecules."
"The rate equation for this reaction is v0 = k(K1K2CA·CB) / (1 + K1CA + K2CB)^2."
"When the experimental rate equation has been determined, it can be useful for deducing the reaction mechanism."