Kinetics

• why does lowering activation energy increase the rate of reaction?

  • more particles have energy above Ea
  • more frequent successful collisions
• How do catalysts work?

  lower activation energy by providing an alternative route for the energy to take
• what is the definition of a catalyst?

  substances that increase rate of reaction without being used up
• How does increasing surface area affect the rate of reaction?

  • More particles exposed
  • more frequent successful collisions
  • rate of reaction increases
• Explain how increasing concentration affect the rate of reaction?

  • More particles per unit of volume
  • more frequent successful collisions
  • rate of reaction increases
• What does the Maxwell-Boltzmann distribution show?

  the spread of energies that molecules of gas have at a particular temperature
• What is the effect of increasing temperature on the rate of reaction?

  • particles have increased kinetic energy
  • many more particles have E>=Ea
  • more frequent successful collisions
  • rate of reaction increases
• What is collision theory?

  • reactions can only occur when collisions take place between particles that have sufficient energy
  • energy needed to break bonds in reactants
  • minimum energy is called the activation energy
• Define activation energy

  the minimum energy which particles need to collide to start a reaction
• Define rate of reaction

  the change in concentration of a substance in unit time