"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."
The power to which the concentration of a reactant is raised in the rate law.
Reactant concentration: The rate of a chemical reaction depends on the concentration of the reactants.
Rate of reaction: The rate of reaction measures how quickly products are formed or reactants are consumed.
Reaction order: The order of a chemical reaction determines how the rate of reaction changes with different concentrations of reactants.
Rate law: The rate law is an equation that relates the rate of a reaction to the concentrations of its reactants.
Rate constant: The rate constant is a proportionality constant in the rate law that measures how quickly a chemical reaction occurs.
Temperature dependence: The rate of a chemical reaction generally increases with temperature because higher temperatures increase the energy and frequency of molecular collisions.
Catalysis: A catalyst is a substance that speeds up a chemical reaction without being consumed itself.
Reaction mechanism: The series of elementary reactions that occur during a complex chemical reaction.
Reaction rate expression: The mathematical expression that describes the rate of a chemical reaction in terms of the concentrations of its reactants.
Half-life: The time it takes for half of the reactants to be consumed in a chemical reaction.
Differential rate law: The rate law expressed in terms of instantaneous rates rather than average rates.
Integrated rate law: An equation that relates the concentration of a reactant to time in a chemical reaction.
Order of reaction with respect to a reactant: The exponent in the rate law that corresponds to the concentration of a specific reactant.
Reaction order with respect to time: The relationship between the concentration of a reactant and time in a chemical reaction.
Concentration-time graphs: Graphs that show the changes in concentration of reactants or products over time in a chemical reaction.
Arrhenius equation: A relationship between the rate constant of a chemical reaction and the activation energy and temperature.
Zero order reaction: A reaction is said to be of zero order if the rate of reaction is independent of the concentration of reactants.
First order reaction: A reaction is said to be of first order if the rate of reaction is directly proportional to the concentration of only one reactant.
Second order reaction: A reaction is said to be of second order if the rate of reaction is directly proportional to the concentration of two reactants or the square of the concentration of a single reactant.
Third order reaction: A reaction is said to be of third order if the rate of reaction is directly proportional to the concentration of three reactants or the cube of the concentration of a single reactant.
Fractional order reaction: A reaction can exhibit fractional order if its rate depends on the concentration of the reactants raised to a non-integer power.
Overall order of reaction: The overall order of a reaction is the sum of the exponents in the rate law.
Complex reaction: A complex reaction is a reaction involving several elementary reactions occurring simultaneously or consecutively.
Pseudo-first order reaction: A reaction is said to be pseudo-first order if the rate of reaction depends on the concentration of only one reactant, even though the reaction is actually second or higher order. This can occur when one of the reactants is present in excess.
Unimolecular reaction: A unimolecular reaction is a reaction where the rate depends only on the concentration of one reactant.
Bimolecular reaction: A bimolecular reaction is a reaction where the rate depends on the concentration of two reactants.
"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."