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