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| activated complex | (also, transition state) unstable combination of reactant species representing the highest energy state of a reaction system
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| activation energy (Ea) | energy necessary in order for a reaction to take place
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| Arrhenius equation | mathematical relationship between the rate constant and the activation energy of a reaction
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| average rate | rate of a chemical reaction computed as the ratio of a measured change in amount or concentration of substance to the time interval over which the change occurred
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| bimolecular reaction | elementary reaction involving the collision and combination of two reactant species
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| catalyst | substance that increases the rate of a reaction without itself being consumed by the reaction
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| collision theory | model that emphasizes the energy and orientation of molecular collisions to explain and predict reaction kinetics
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| elementary reaction | reaction that takes place precisely as depicted in its chemical equation
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| frequency factor (A) | proportionality constant in the Arrhenius equation, related to the relative number of collisions having an orientation capable of leading to product formation
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| half-life of a reaction (tl/2) | time required for half of a given amount of reactant to be consumed
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| heterogeneous catalyst | catalyst present in a different phase from the reactants, furnishing a surface at which a reaction can occur
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| homogeneous catalyst | catalyst present in the same phase as the reactants
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| initial rate | instantaneous rate of a chemical reaction at t = 0 s (immediately after the reaction has begun)
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| instantaneous rate | rate of a chemical reaction at any instant in time, determined by the slope of the line tangential to a graph of concentration as a function of time
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| integrated rate law | equation that relates the concentration of a reactant to elapsed time of reaction
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| intermediate | molecule or ion produced in one step of a reaction mechanism and consumed in another
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| method of initial rates | use of a more explicit algebraic method to determine the orders in a rate law
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| molecularity | number of reactant species (atoms, molecules or ions) involved in an elementary reaction
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| overall reaction order | sum of the reaction orders for each substance represented in the rate law
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| rate constant (k) | proportionality constant in the relationship between reaction rate and concentrations of reactants
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| rate expression | mathematical representation relating reaction rate to changes in amount, concentration, or pressure of reactant or product species per unit time
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| rate law | (also, rate equation) mathematical equation showing the dependence of reaction rate on the rate constant and the concentration of one or more reactants
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| rate of reaction | measure of the speed at which a chemical reaction takes place
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| rate-determining step | (also, rate-limiting step) slowest elementary reaction in a reaction mechanism; determines the rate of the overall reaction
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| reaction mechanism | stepwise sequence of elementary reactions by which a chemical change takes place
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| reaction order | value of an exponent in a rate law, expressed as an ordinal number (for example, zero order for 0, first order for 1, second order for 2, and so on)
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| termolecular reaction | elementary reaction involving the simultaneous collision and combination of three reactant species
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| unimolecular reaction | elementary reaction involving the rearrangement of a single reactant species to produce one or more molecules of product
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