Learn why are some chemical reactions energetically favorable but very slow to happen?
Reaction
Rates
Why
are some reactions
energetically favorable but very slow to happen? This question is answered in
the program Reaction Rates. The general concept of rate is introduced with
numerical examples and sets the stage for an understanding of reaction rates.
Factors that affect reaction rates, such as temperature and concentration, are
explained through the concepts of collision theory and activation energy. A
step-by-step approach teaches rate laws and is reinforced with interactive
lessons covering both rate constants and reaction order. The program also
covers reaction mechanisms, including the rate-determining step. Throughout
the program, videos and animations help students visualize what happens at the
particle level and illustrate the incisive analogies.
OUTLINE:
I. Introduction
II. Rates of Reactions A. The Concept of Rates 1.
The Definition of Rate 2.
Examples of Rates 3.
Converting Units of Time B. Reaction Rates 1.
General Characteristics 2.
Measuring the Change in
Concentration 3.
Stoichiometry and Reaction
Rates a.
Determining Concentration Through Stoichiometry 4.
Definition of Reaction Rate
a.
Normalizing the Reaction
Rate 5.
Calculating Reaction Rate 6.
Change in Reaction Rate
as the Reaction Proceeds 7.
Instantaneous vs. Average
Rates
III. Factors Affecting Reaction Rates A. Nature of Reactants B. Temperature C. Catalysts 1.
Enzymes D. Surface Area E. Concentration
IV. Collision Theory A. Kinetic Energy 1.
Particles in a Sample Have
Different Kinetic Energy B. Activation Energy 1.
A Visual Demonstration of
Activation Energy C. Why Increasing Temperature
Increases Reaction
Rates D. The Activated Complex E. Catalysts 1.
Catalysts Lower Activation
Energy
V. Rate Laws A.
Rate is Proportional to the Concentration
of Reactants B. Definition of Rate Law C. Calculating the Rate Constant 1.
An Example 2.
Another Example D. Reaction Order 1.
Determining Reaction Order a.
Example Using Sulfuryl Chloride b.
Example Using Hydrogen
Iodide c.
Example Using Nitrogen Dioxide
VI. Reaction Mechanisms A. Reactions Occur in Multiple Steps
B. The Steps of a Reaction Mechanism
are Elementary Processes C. An Example of a Reaction Mechanism
D. Rate Laws and Elementary Processes* 1.
Determining Rate Laws From
Elementary Processes* E. The Rate-Determining Step F. Evaluating Reaction Mechanisms*
1.
An Example* G. Conclusion 1.
Reviewing the Reaction of
Carbon Monoxide and
Oxygen 2.
Conclusion
*More advanced topics
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A. The Concept of Rates
