Kinetics


 * __Introduction__**

Kinetics is all about the rate (or speed) at which chemical reactions occur. Explosions are an example of very rapid reactions while rusting is very slow. The rate of a reaction can be determined by considering the change in concentration of the reactants disappearing over time or the appearance of products over time. This unit will look at these calculations and consider some of the factors that affect reaction rates.



__**Activation Energy**__

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__**Reaction Rates**__ Go to [] for a simulation of reaction rates. Follow the instructions and answer the question in you notebook.

__**Collision Theory**__

Go to [|www.explorelearning.com] and work through the "Collision Theory" gizmo and answer the student worksheet questions.

__**Kinetic molecular Theory**__ An animation of average kinetic energy as a function of temperature --> here

__**Maxwell-Boltzman Distribution**__

Go to [] and click "Run/Save the Kinetic Theory Particle Simulations" link.
 * 1) Run simulations 1, 2 and 3.
 * 2) Enter at least 5 different values into each simulation
 * 3) Plot the value for the maximum of each curve vs the variable you are changing (e.g. temperature)
 * 4) Draw conclusions about what the M-B Distribution curves are showing and what your graphs are showing.

__**Reaction Order**__

Go to [] and use the simulation to discover how to determine the order of a reaction. (Remember, you can only determine reaction order experimentally...or by an experimental simulation like this one)