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K & E

Regents Chem - Kinetics & Equilibrium

QuestionAnswer
Activation energy energy required to take reactants or products to the top of a potential energy diagram. Every reaction has activation energy
Spontaneous reaction process that occurs on its own, without outside involvement. Usually exothermic (negative delta H) and increase in entropy (positive delta S)
Chemical Equilibrium rates of forward and reverse reactions are equal. Concentrations are constant.
Solution equilibrium in a saturated solution when rate of dissolving equals rate of crystallization
Phase equilibrium in a closed container, rate of evaporation equals rate of condensation. If container is NOT closed, the gas will just escape.
LeChatlier’s Principle when a stress is placed on a system at equilibrium, one direction will be favored so that the stress can be alleviated.
Keq Equilibrium constant expression. Concentration of products divided by concentration of reactants. Coefficients become exponenets
Effect on equilibrium of increasing reactant concentration shift to product side. More products are made but reactants decrease.
Effect on equilibrium of adding a catalyst a catalyst has NO EFFECT on EQUILIBRIUM!
Effect on equilibrium of increasing temperature shift away from the heat (kJ). The shift is in the endothermic direction
Effect on equilibrium of decreasing temperature shift to the side with the heat…this will raise the temperature back up.
Effect on equilibrium of increase in pressure shift to the side with less moles. Less stuff can fit better in a smaller container.
Enthalpy heat content of a system
Entropy measure of the disorder or chaos of a system
Effect of a catalyst on collisions and reaction rate provides another mechanism for the reaction with less activation energy so more collisions are effective
Effect of a increase in temp on collisions and reaction rate more collisions, more effective collisions, increased rate (it takes less time)
Effect of a increase in surface area on collisions and reaction rate more collisions, more effective collisions, increased rate (it takes less time)
2 factors needed in order for collisions to be effective proper kinetic energy and proper orientation
Created by: etucci