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OpenStax Chem 12
This content is available for free at http://cnx.org/content/col11760/1.9
| Term | Definition |
|---|---|
| activated complex | (also, transition state) unstable combination of reactant species representing the highest energy state of a reaction system |
| activation energy (Ea) | energy necessary in order for a reaction to take place |
| Arrhenius equation | mathematical relationship between the rate constant and the activation energy of a reaction |
| 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 |
| bimolecular reaction | elementary reaction involving the collision and combination of two reactant species |
| catalyst | substance that increases the rate of a reaction without itself being consumed by the reaction |
| collision theory | model that emphasizes the energy and orientation of molecular collisions to explain and predict reaction kinetics |
| elementary reaction | reaction that takes place precisely as depicted in its chemical equation |
| 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 |
| half-life of a reaction (tl/2) | time required for half of a given amount of reactant to be consumed |
| heterogeneous catalyst | catalyst present in a different phase from the reactants, furnishing a surface at which a reaction can occur |
| homogeneous catalyst | catalyst present in the same phase as the reactants |
| initial rate | instantaneous rate of a chemical reaction at t = 0 s (immediately after the reaction has begun) |
| 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 |
| integrated rate law | equation that relates the concentration of a reactant to elapsed time of reaction |
| intermediate | molecule or ion produced in one step of a reaction mechanism and consumed in another |
| method of initial rates | use of a more explicit algebraic method to determine the orders in a rate law |
| molecularity | number of reactant species (atoms, molecules or ions) involved in an elementary reaction |
| overall reaction order | sum of the reaction orders for each substance represented in the rate law |
| rate constant (k) | proportionality constant in the relationship between reaction rate and concentrations of reactants |
| rate expression | mathematical representation relating reaction rate to changes in amount, concentration, or pressure of reactant or product species per unit time |
| 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 |
| rate of reaction | measure of the speed at which a chemical reaction takes place |
| rate-determining step | (also, rate-limiting step) slowest elementary reaction in a reaction mechanism; determines the rate of the overall reaction |
| reaction mechanism | stepwise sequence of elementary reactions by which a chemical change takes place |
| 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) |
| termolecular reaction | elementary reaction involving the simultaneous collision and combination of three reactant species |
| unimolecular reaction | elementary reaction involving the rearrangement of a single reactant species to produce one or more molecules of product |
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point4christ
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