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Kinetics

Kinetics. Answers question, “How fast?” Rate is proportional to the concentration of reactants raised to a power. Rate law is experimentally determined. =>. =>. Activation Energy. Minimum energy required to reach the transition state .

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Kinetics

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  1. Kinetics • Answers question, “How fast?” • Rate is proportional to the concentration of reactants raised to a power. • Rate law is experimentally determined.=>

  2. => Activation Energy • Minimum energy required to reach the transition state. • At higher temperatures, more molecules have the required energy.

  3. => Reaction-Energy Diagrams • For a one-step reaction:reactants  transition state  products • A catalyst lowers the energy of the transition state.

  4. Rate-Limiting Step • Reaction intermediates are stable as long as they don’t collide with another molecule or atom, but they are very reactive. • Transition states are at energy maximums. • Intermediates are at energy minimums. • The reaction step with highest Ea will be the slowest, therefore rate-determining for the entire reaction. =>

  5. => Energy Diagram for a Two-Step Reaction • Reactants  transition state  intermediate • Intermediate  transition state  product

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