Chemical Kinetics

intermediate configuration of atoms during a chemical reaction with high potential energy

minimum energy needed for a chemical reaction to initiate

equation that relates temperature to the rate constant; given as $k=Ae^{-\frac{E_a}{RT}}$

elementary reaction that occurs between two reactants

substance that causes the rate of a chemical reaction to increase

field that studies the rates of chemical reactions

theory that describes how chemical reactions occur through molecular collisions and why reaction rates vary between reactions

reaction that takes place in a single step

biological molecule that catalyzes a biological reaction

reaction in which the rate is dependent on the concentration of one of the reactants, raised to the power of one; given as a rate law with the form $r=k\lbrack\rm{A}\rbrack$

catalyst that is in a different phase than that of the reactants

catalyst that is in the same phase as that of the reactants and is present in the reaction medium

rate of a chemical reaction at a particular moment

rate law that defines concentration as a function of time

species that is produced in one step and consumed in another step of a chemical reaction

number of molecules that participate in the rate-determining step of a chemical reaction

constant relating reaction rate to concentrations of reactants

mathematical expression that relates rate with a rate constant and concentrations of the reactants; given as the general form $r=k\lbrack{\rm{A}}\rbrack^m\lbrack{\rm{B}}\rbrack^n$

slowest reaction in a multistep reaction that determines the overall rate

time it takes for a reactant to drop to half its starting concentration during a chemical reaction

exact step or steps required to convert reactants into products

sum of the powers that the reactant concentrations are raised to in the rate expression

speed at which a reaction occurs

reaction in which the sum of the powers that the reactant concentrations are raised to in the rate expression is equal to two; given as a rate law with the form $r=k\lbrack{\rm A}\rbrack\lbrack{\rm B}\rbrack$ or $r=k\lbrack{\rm A}\rbrack^2$

elementary reaction that occurs between three reactants

elementary reaction with one reactant

reaction in which rate is not dependent on reactant concentrations; given as a rate law with the form $r=k$