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| the change in the concentration of reactants or products per unit of time. | ||
| the reaction rate at a particular time as opposed to the average rate over an interval of time | ||
| the instantaneous rate at t=0 | ||
| Rate = k[A]^m[B]^n | ||
| a constant of proportionality between the reaction rate and the concentrations of reactants that appear in the rate law | ||
| the power to which the concentration of a reactant is raised | ||
| the sum of the reaction orders of all the reactants appearing in the rate expression when the rate can be expressed as (rate = k[a]^m[B]^n | ||
| a reaction in which the reaction rate is proportional to the concentration of a single reactant raised to the first power | ||
| the time required for the concentration of a reactant substance to decrease to half its initial value | ||
| a reaction in which the overall reaction order (the sum of the concentration-term exponents) in the rate law is 2 | ||
| a model of reaction rates based on the idea that molecules must collide to react; it explains the factors influencing reaction rates in terms of the frequency of collisions, the number of collisions with energies exceeding the activation energy, and the probability that the collisions occur with suitable orientations | ||
| the minimum energy needed for reaction; the height of the energy barrier to formation of products | ||
| the particular arrangement of atoms found at the top of the potential-energy barrier as a reaction proceeds from reactants to products | ||
| an equation that relates the rate constant for a reaction to the frequency factor, A, the activation energy and the temperature | ||
| a term in the Arrhenius equation that is related to the frequency of collision and the probability that the collisions are favourable oriented for reaction | ||
| a detailed picture, or model, of how the reaction occurs; that is, the order in which bonds are broken and formed and the changes in relative positions of the atoms as the reaction proceeds | ||
| a process in a chemical reaction that occurs in a single event or step. An overall chemical reaction consists of one or more of these. | ||
| the number of molecules that participate as reactants in an elementary reaction | ||
| an elementary reaction that involves a single molecule | ||
| an elementary reaction that involves two molecules | ||
| an elementary reaction that involves three molecules. | ||
| a substance formed in one elementary step of a multistep mechanism and consumed in another; it is neither a reactant nor an ultimate product of the overall reaction | ||
| the slowest elementary step in a reaction mechanism | ||
| a catalyst that is in the same phase as the reactant substances | ||
| a catalyst that is in a different phase as the reactant substances | ||
| the binding of molecules to a surface | ||
| a protein molecule that acts to catalyze specific biochemical reactions | ||
| specific site on a heterogeneous catalyst or an enzyme where catalysis occurs | ||
| a substance that undergoes a reaction at the active site in a n enzyme | ||
| a model of enzyme action in which the substrate molecule is pictured as fitting rather specifically into the active site on the enzyme. it is assumed that in being bound to the active site, the substrate is somehow activated for reaction |
