| Term | Definition |
|---|
| Rates | describes the speed of change over an interval of time |
| Collision Theory | atoms, ions, and molecules can react to form products when they collide, provided that the particles have enough kinetic energy |
| Activation Energy | the minimum energy colliding particles must have in order to react |
| Activated Complex | an unstable arrangement of atoms that exists momentarilly at the peak of the activation-energy barrier; an intermediate or transitional structure formed during the course of a reaction |
| Transition State | a term sometimes used to refer to the activated complex |
| Catalyst | a substance that increases the rate of reaction by lowering the activation-energy barrier; the catalyst is not used up |
| Inhibitor | a substance that interferes with the action of a catalyst |
| Reversible Reactions | a reaction in which the conversion of reactants to products and the conversion of products to reactants occur simultaneously |
| Chemical Equilibrium | a state of balance in which forward and reverse reactions are taking place at the same rate; no net change in the amounts of reactants and products occures in the chemical system |
| Equilibrium Position | the relative concentrations of reactants and products of a reaction that has reached equilibrium; indicates whether the reactants or products are favored in the reversible reaction |
| Le Chatelier's Principle | whe stress is applied to a system at equilibrium, the system changed to relieve the stress |
| Equilibrium Constant (Keq) | The ratio of product concentrations to reactant concentrations at equilibrium with each concentration raised to a power equal to the number of moles of that substance in the balanced chemical equation |
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