Collision theory

• What is the definition of rate in the context of kinetics?

  Rate is the change in concentration or amount of a reactant or product per unit time.
• What must happen for a reaction to occur according to collision theory?

  Particles must collide with the right orientation and sufficient energy.
• What is activation energy?

  Activation energy is the minimum amount of energy required for a reaction to occur.
• How is activation energy represented in an energy profile diagram?

  It is represented as the difference between the energy of the reactants and the peak of the reaction profile line.
• How does the activation energy of reactions with low activation energy compare to those with high activation energy?

  Reactions with low activation energy require less energy to break bonds compared to those with high activation energy.
• How can reaction conditions be altered to increase the likelihood of successful collisions?


  By providing the particles with more energy through changes in conditions.
• What is the role of activation energy in chemical reactions?

  It is the minimum energy required for a reaction to occur.