var nc = 29, fc = new Array(nc); fc[0] = {t:"Activated Complex",d:"A species formed in a chemical reaction when molecules have enough energy to react with each other."}; fc[1] = {t:"Activation Energy (Ea)",d:"The minimum energy molecules need to react when they collide."}; fc[2] = {t:"Arrhenius Equation",d:"Relates the rate constant of a reaction to absolute temperature (T), the activation energy of the reaction (Ea), and the frequency factor (A)."}; fc[3] = {t:"Bimolecular Step",d:"A step in a reaction mechanism involving a collision between two molecules."}; fc[4] = {t:"Catalyst",d:"A substance added to a reaction that increases the rate of the reaction but is not consumed in the process."}; fc[5] = {t:"Chemical Kinetics",d:"The study of the rates of change of concentrations of substances involved in chemical reactions."}; fc[6] = {t:"Elementary Step",d:"A molecular-level view of a single process taking place in a chemical reaction."}; fc[7] = {t:"Energy Profile",d:"Graph showing the changes in potential energy for a reaction as a function of the progress of the reaction from reactants to products."}; fc[8] = {t:"Frequency Factor (A)",d:"The product of the frequency of molecular collisions and a factor that expresses the probability that the orientation of the molecules is appropriate for a reaction to occur."}; fc[9] = {t:"Half-Life (t1/2)",d:"The time in the course of a chemical reaction during which the concentration of a reactant decreases by half."}; fc[10] = {t:"Heterogeneous Catalyst",d:"A catalyst in a phase different than the reactants."}; fc[11] = {t:"Homogeneous Catalyst",d:"A catalyst in the same phase as the reactants."}; fc[12] = {t:"Initial Rate",d:"The rate of a reaction at t = 0, immediately after the reactants are mixed."}; fc[13] = {t:"Instantaneous Rate",d:"The rate of a reaction at a specific instant during the course of the reaction."}; fc[14] = {t:"Integrated Rate Law",d:"A mathematical expression that describes the change in concentration of a reactant in a chemical reaction with time."}; fc[15] = {t:"Intermediate",d:"A species produced in one step of a reaction and consumed in a subsequent step."}; fc[16] = {t:"Molecularity",d:"The number of ions, atoms, or molecules involved in an elementary step in a reaction."}; fc[17] = {t:"Overall Reaction Order",d:"The sum of the exponents of the concentration terms in the rate law."}; fc[18] = {t:"Photochemical Smog",d:"A mixture of gases formed in the lower atmosphere when sunlight interacts with compounds produced in internal combustion engines and other pollutants."}; fc[19] = {t:"Pseudo-First-Order",d:"A reaction in which all the reactants but one are present at such high concentrations that they do not decrease significantly during the course of the reaction, so that reaction rate is controlled by the concentration of the limiting reactant."}; fc[20] = {t:"Rate Constant",d:"The proportionality constant that relates the rate of a reaction to the concentrations of reactants."}; fc[21] = {t:"Rate Law",d:"An equation that defines the experimentally determined relation between the concentrations of reactants in a chemical reaction and the rate of that reaction."}; fc[22] = {t:"Rate-Determining Step",d:"The slowest step in a multistep chemical reaction."}; fc[23] = {t:"Reaction Mechanism",d:"A set of steps that describe how a reaction occurs at the molecular level; the mechanism must be consistent with the rate law for the reaction."}; fc[24] = {t:"Reaction Order",d:"An experimentally determined number defining the dependence of the reaction rate on the concentration of a reactant."}; fc[25] = {t:"Reaction Rate",d:"How rapidly a reaction occurs; it is related to rates of change in the concentrations of reactants and products over time."}; fc[26] = {t:"Termolecular Step",d:"A step in a reaction mechanism involving a collision among three molecules."}; fc[27] = {t:"Transition State",d:"A high-energy state between reactants and products in a chemical reaction."}; fc[28] = {t:"Unimolecular Step",d:"A step in a reaction mechanism involving only one molecule on the reactant side."};