| second-order kinetics | A term describing the reaction rate of a chemical reaction in which the rate is proportional to the product of the concentrations (in moles) of two of the reactants (also called bimolecular kinetics), or to the square of the molar concentration of the reactant if there is only one. Such a reaction might have an equation like rate = k[A][B] or rate = k[A]2, where k is the reaction rate constant, [A] is the concentration of reactant A, and [B] is the concentration of reactant B. (09 Oct 1997) |
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| third-order kinetics | <pharmacology> A term describing the reaction rate of a chemical reaction in which the rate is proportional to the product of the concentrations (in moles) of three of the reactants, the product of the molar concentration of one reactant and the square of the molar concentration of another reactant, or the cube of the molar concentration of one of the reactants. Such a reaction might have an equation like rate = k[A][B][C] or rate = [A][B]2 or rate = [A]3, where k is the reaction rate constant, [A] is the concentration of reactant A, [B] is the concentration of reactant B, and [C] is the concentration of reactant C. (09 Oct 1997) |
| kinetics | <physics> See Dynamics. Source: Websters Dictionary (01 Mar 1998) |
| first-order kinetics | A term describing the reaction rate of a chemical reaction in which the rate is proportional to the concentration (in moles) of only one of the reactants. Such a reaction might have an equation like rate = k[A], where k is the reaction rate constant and [A] is the concentration of a reactant A. (09 Oct 1997) |