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Review Chapter 12 - Kinetics

This review Chapter 12 - Kinetics

Delilah Narvaez

on 8 April 2014

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Transcript of Review Chapter 12 - Kinetics

Lets Review Kinetics
Things that Affect Reaction Rate
Surface Area
Concentration of Reactants
Increasing Pressure
What State of Matter?
At the top of the curve, the bonds in the reactants have been broken.
The amount of energy put in to break these bonds
Is called the activation energy
Step 1 R-Br --> R+ + Br- slow
Step 2 R+ + OH- --> R-OH fast

* R = some alkyl group
The activation energy is the minimum amount of energy needed for the reaction to occur.
A catalyst may work by lowering the activation energy for a reaction.
Increasing the temperature of a reaction increases the kinetic energy of the particles which increases the number of collisions so the reaction rate increases.
Increasing the concentration of reactants in solution increases the number of reactant particles which increases the number of collisions so the reaction rate increases.
Rate of Stirring
Stirring keeps reactant particles in motion increasing the chances of collision and increasing the rate of reaction.
Energy Profile?
Draw one
Is it Endothermic or Exothermic?
Label it, then draw the other and label.
When are collisions effective?
Correct Orientation
Enough Energy
Possible Catalysts
Write the rate law
T2 > T1
Enzymes in metabolic pathways
1. A metabolic pathway is a series of chemical reactions that use the products of the previous reaction as the reactants for
the next reaction
2. The products of one reaction can become an inhibitor of any of the previous reactions. Usually they are the final
products (negative feedback)
Are there any Intermediates?
Zero Order Proven
1st order Ln[A] versus time
ln [A]
2nd Order 1/[A] versus Time
Full transcript