Reaction rates -chemistry

• Who is the presenter of the video on reaction rates?

  Chris Harris
• Where can the slides used in the video be purchased?

  In the description box below
• What is the purpose of the video on reaction rates?

  It provides an overview for OCR revision
• What does the rate of reaction measure?

  Change in concentration per unit time
• How is the rate of reaction calculated?

  Amount of reactant used divided by time
• What must happen for a reaction to occur according to collision theory?

  Particles must collide in the right direction
• What is activation energy?

  Minimum energy required for a reaction
• What does an energy profile diagram show?

  Changes in energy during a reaction
• How does the shape of the energy profile relate to activation energy?

  Activation energy is the peak between reactants and products
• What happens to molecules as they gain kinetic energy?

  Their bonds begin to stretch
• What does the Maxwell-Boltzmann distribution illustrate?

  Energy distribution in gas particles
• What does the peak of the Maxwell-Boltzmann distribution represent?

  Most likely energy of a particle
• What does the area under the Maxwell-Boltzmann curve represent?

  Total number of molecules in the sample
• What happens to the rate of reaction when temperature increases?

  More particles have energy above activation energy
• How does increasing pressure affect the rate of reaction?

  Particles are closer, leading to more collisions
• What is the effect of increasing concentration on reaction rate?

  Increases frequency of collisions between particles
• What is a catalyst?

  Substance that increases reaction rate
• How does a catalyst lower activation energy?

  Provides an alternative reaction pathway
• What is a heterogeneous catalyst?

  Catalyst in a different phase than reactants
• What is the role of zeolite as a catalyst?

  Increases surface area for reactions
• What factors affect the rate of reaction?

  • Temperature
  • Pressure
  • Concentration
  • Presence of catalysts
• What are the differences between homogeneous and heterogeneous catalysts?

  Homogeneous:

  • Same phase as reactants
  • Example: liquid catalysts

  
  

  Heterogeneous:

  • Different phase than reactants
  • Example: solid catalysts in gas reactions
• What are the implications of using catalysts in industrial processes?

  • Speeds up reactions
  • Reduces energy costs
  • Increases efficiency
  • Saves time and money
• What is the significance of activation energy in chemical reactions?

  • Determines the rate of reaction
  • Higher activation energy means slower reactions
  • Lower activation energy means faster reactions
• How does temperature influence the kinetic energy of particles?

  • Higher temperature increases kinetic energy
  • More energetic collisions occur
  • Leads to faster reaction rates
• What is the relationship between collision theory and reaction rates?

  • More collisions lead to higher reaction rates
  • Proper orientation and energy are necessary
  • Collision theory explains how reactions occur
• What are the tiny microscopic pores called that increase the surface area of a catalyst?

  Micropores
• How do micropores affect reactions on a catalyst?

  They allow reactions to happen quicker
• What is a zeolite?

  A type of catalyst with micropores
• What are the two types of catalysts mentioned?

  Homogeneous and heterogeneous
• What does "heterogeneous" mean in the context of catalysts?

  They are in a different phase than reactants
• What is the Haber process used for?

  Manufacturing ammonia
• What type of catalyst is used in the Haber process?

  Iron catalyst
• How does a solid catalyst speed up a reaction?

  By providing an alternative pathway
• How can the surface area of a solid catalyst be increased?

  By grinding it into a powder
• What is a characteristic of homogeneous catalysts?

  They are in the same phase as reactants
• What happens to a homogeneous catalyst during a reaction?

  It is used up and then reformed
• How do heterogeneous catalysts function differently from homogeneous catalysts?

  They are not used up in the reaction
• How do catalysts affect the activation energy of a reaction?

  They lower the activation energy
• What does the Boltzmann distribution show when a catalyst is present?

  More particles have enough energy to react