| INTRODUCTION
TO KINETICS |
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Chemical kinetics |
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Importance of the study of chemical
kinetics |
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Application
to industrial processes |
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Application to everyday processes |
| REACTION
RATES |
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Description |
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Factors affecting reaction rate |
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The concentration of reactants |
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The temperature at which the reaction occurs |
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The
presence of a catalyst |
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The surface area of a solid or liquid reactant
or catalyst |
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Definition |
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Verbal definition |
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Mathematical definition |
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Two
approaches to describing reaction rate |
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Average rate |
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Instantaneous rate |
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Graphical representations of
reaction rate |
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Relating rate of disappearance of a
reactant and rate of appearance of a product from the balanced equation |
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Determining the average reaction
rate from concentration measurements at specific times |
| DEPENDENCE
OF REACTION RATE ON CONCENTRATION |
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Rate constant |
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Definition |
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Symbol |
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Characteristics |
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Rate law |
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Definition |
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Form |
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Reaction order |
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For a reactant (or catalyst) |
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For a reaction |
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Examples |
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Determining the rate law from
initial concentrations and initial rates |
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Procedure |
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Examples |
| CHANGES
OF CONCENTRATION WITH TIME |
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The use for a rate law |
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The use for a concentration-time
law |
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Concentration-time laws for first
order and second order reactions |
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First order reactions:
concentration-time equation |
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Second
order reactions: concentration-time
equation |
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Using
graphing to determine the order of a reaction |
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An alternative to the approach of
running multiple experiments |
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Approach |
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First order assumption |
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Second order assumption |
| COLLISION
THEORY |
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Reactions involve collisions
between particles |
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Involve
a transfer of atoms |
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Happens when the particles collide |
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More collisions mean the reaction
will go faster |
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Collisions alone are not a complete
explanation |
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Statistics |
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If every binary collision led to a
product, then every reaction would be over almost instantaneously |
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Energy considerations are also a
part of the explanation |
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Kinetic energy can be converted to vibrational
energy in collisions |
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When the translational kinetic energy of the
colliding particles is high enough |
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When the translational kinetic energy is too
small |
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Collision theory and an energy
description of bond breaking and forming. |
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Activation energy |
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Activated complex |
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Potential energy profiles |
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Collision theory and an explanation
of factors affecting reaction rate |
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The effect of increasing
temperature |
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The effect of increasing
concentration |
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The effect of increasing the
surface area of a solid or liquid reactant |
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The presence of a catalyst |
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The relationship among activation
energy, temperature, frequency of collisions, and the rate law constant |
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Arrhenius equation |
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The comparative Arrhenius equation |
| REACTION
MECHANISMS |
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Definition and description of a
reaction mechanism |
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Definition and description of
elementary steps |
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Definition and description of
reaction intermediate |
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Definition
and description of molecularity |
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Writing the overall balanced
equation from the mechanism |
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Rate laws and elementary steps |
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Rate laws for elementary steps with
each of the three molecularities |
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Writing rate laws for elementary
steps |
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Rate law and mechanisms |
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Rate law and single step mechanisms |
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Rate law and multi-step mechanisms |
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Determining the rate-determining
step from the rate law |
| CATALYSIS
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Importance
of catalysts |
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Industry |
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Biologically |
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Nature of catalysts |
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Catalysts increase the rate of
reaction |
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Catalysts increase the rate of both
the forward and the reverse reaction |
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Catalysts do not undergo permanent
chemical change in the reaction they catalyze |
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Catalysts work by lowering
the activation energy for the reaction -
both forward and reverse |
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Inhibitor |
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Homogeneous catalysis |
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Heterogeneous catalysis |
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Enzyme catalysis |
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