Kinetics

• What must particles do in order to react?

  Collide with sufficient energy (activation energy) and the correct orientation
• Do most collisions result in a reaction?

  No
• Define Activation Energy.


  The minimum energy that particles must collide with for a reaction to occur
• What are the key features of a Maxwell-Boltzman Curve?

  • Average energy
  • Activation energy
  • Most probable energy
  • Effect of increasing temperature (shown in a different color)
• What is the effect of increasing temperature on the rate of reaction?

  Increasing temperature leads to an increased rate of reaction
• Why does increasing temperature increase the rate of reaction?


  Much higher proportion of particles have energy greater than the activation energy, leading to more successful collisions per second

  
• What is the effect of increasing concentration or pressure on the rate of reaction?

  Increased concentration or pressure leads to an increased rate of reaction
• Why does increasing concentration or pressure increase the rate of reaction?

  There are more particles in a given volume, leading to more frequent successful collisions
• What is a catalyst?


  A substance which increases the rate of reaction but is not used up in the reaction
• How do catalysts work to increase the rate of reaction?

  They provide an alternative reaction pathway with a lower activation energy
• How do catalysts affect the energy of particles in a reaction?

  Catalysts lower the activation energy, allowing more particles to have energy greater than the activation energy
• What is the result of more frequent successful collisions due to catalysts?

  Increased reaction rate