Chapter 18 Vocabulary: Reaction Rates and Equilibrium
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| activated complex | The arrangement of atoms at the peak of the activation energy barrier.
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| activation energy (Ea) | The minimum energy colliding particles must have in order to react.
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| transition state | This is what the activated complex is sometimes called.
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| Collision theory | says that atoms, ions, and molecules can form a chemical bond when they collide, provided the particles have enough kinetic energy.
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| catalyst | A substance that increases the rate of a reaction without being used up itself in the reaction.
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| reversible reaction | The reactions in both directions occur simultaneously.
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| chemical equilibrium | This is when the forard and the reverse reactions are taking place at the same time.
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| Le Chatelier's principle | If a stress is applied to a system in a dynamic equilibrium, the system changes to relieve the stress.
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| spontaneous reaction | Naturally favor the formation of products at the specified conditions.
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| nonspontaneous reaction | Do not favor the formation of products at the specified conditions.
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| equilibrium constant (Keq) | The ratio of product concentrations to reactant concentrations, with each concentration raised to a power given by the number of moles of that substance in the balanced chemical equation.
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| entropy | Of a liquid or solid substance at 25 degrees celcius and 101.3 kPa is designated S^o
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| Reaction Rate | Speed at which a chemical reaction proceeds, in terms of amount of product formed or amount of reactant consumed per unit of time.
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| solubility product constant (Ksp) | Is equal to the product of the concentration terms each raised to the power of the coefficient of the substance in the dissociation equation.
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| enthalpy | The amount of heat that a substance has at a given temperature or pressure.
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| potential energy diagram | shows how energy changes during the course of a chemical reaction.
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