Physical chemistryLesson 6 of 6 in the course Kinetics

Catalysis: Reaction Pathways, Ozone Chemistry, Surfaces, and Enzymes

5 flashcards · 5 quiz questions · 5 match pairs · 5 fill-in sentences · English

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Summary

Catalysts increase reaction rates by providing an alternative reaction pathway. Understanding energy diagrams and reaction mechanisms explains how they do this without changing the overall reaction.

A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the overall reaction. It participates in reaction steps, but is regenerated by the end of the catalytic process.

All flashcards

Catalyst
A substance that increases reaction rate and is regenerated rather than consumed overall.
Activation energy
The energy difference between a step's reactants and its transition state.
Heterogeneous catalyst
A catalyst in a different phase from its reactants, often acting at a surface.
Enzyme-substrate complex
A reaction intermediate formed when a substrate binds to an enzyme's active site.
Oxidoreductase
An enzyme class that catalyzes oxidation-reduction reactions.

Quiz questions

  1. What defines a homogeneous catalyst?Answer: It is in the same phase as the reactants.
  2. What is the net reaction for nitric oxide-catalyzed ozone decomposition in the mechanism with steps NO + O₃ → NO₂ + O₂, O₃ → O₂ + O, and NO₂ + O → NO + O₂?Answer: 2O₃ → 3O₂
  3. Which sequence describes the typical stages of heterogeneous surface catalysis?Answer: Adsorption, activation, surface reaction, desorption
  4. What does the induced-fit model propose about enzyme-substrate binding?Answer: The enzyme changes shape as it binds the substrate.
  5. Reactants have an energy of 6 kJ and a transition state has an energy of 20 kJ. What is the activation energy?Answer: 14 kJ

Based on Chemistry 2e by Paul Flowers, Klaus Theopold, Richard Langley, William R. Robinson, PhD (OpenStax), licensed CC BY 4.0. Adapted into a summary, flashcards and quizzes.

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