KINETICS

• Rate of Reaction

  amount of product formed over time/ amount of reactant used up over time
• Collision Theory

  Successful collisions happen when particles’ energy is greater than the activation energy and they collide in the correct orientation.
• How does increasing the concentration affect the rate of reaction?

  Increases
• How does increasing the pressure affect the rate of reaction?

  Increases
• How does increasing the surface area affect the rate of reaction?

  Increases
• How does increasing the temperature affect the rate of reaction?

  Increases
• How does a catalyst affect the rate of reaction?

  Increases
• • Increasing concentration increases the number of particles per unit volume
  • More successful collisions per unit time
  • Increases rate of reaction
• • Increasing pressure decreases volume
  • Increases number of particles per unit volume
  • More successful collisions per unit time
  • Increases rate of reaction
• • Decreasing the particle size reveals more surface for other reagent to react with
  • More successful collisions per unit time
  • Increases rate of reaction
• • Increasing temperature means more particles have energy greater than the activation energy
  • Increases collision frequency
  • More successful collisions per unit time
  • Increases rate of reaction
• • Catalysts provide alternative route with a lower activation energy
  • More particles have energy greater than activation energy
  • More successful collisions per unit time
  • Increases rate of reaction
• What is on y axis in Maxwell-Boltzmann Distribution graph?

  Number of particles
• What is on x axis in Maxwell-Boltzmann Distribution graph?

  Energy
• Ea

  Activation energy
• Emp

  Most probable energy
• Why does the M-B graph start at the origin?

  no particles have 0 energy
• Why does the M-B graph not reach x axis?

  There is no maximum energy
• What does the total area under the curve represent?

  Total amount of particles in a system
• What particles are to the right of the Ea?

  Particles with the minimum energy needed to collide successfully
• If the second curve is higher than the first curve it is a lower temperature
• If the second curve is smaller than the first curve the temperature is higher