collision theory

• What does collision theory explain about reaction rates?

  It explains how collisions affect reaction rates
• What are the two main factors that affect the rate of a chemical reaction according to collision theory?

  Collision frequency and energy transferred
• What is the minimum energy required for particles to react called?

  Activation energy
• What happens during a successful collision?

  Particles react to form products
• How does increasing the number of collisions affect the rate of reaction?

  It increases the rate of reaction
• What effect does increasing temperature have on particle movement?

  Particles move faster
• How does increased temperature affect collision frequency?

  It increases the collision frequency
• What happens to the energy of collisions when temperature increases?

  Energy of collisions increases
• Why do reactions happen more quickly at higher temperatures?

  More successful collisions occur
• What are the three factors that lead to an increased rate of reaction?

  • Increasing temperature
  • Increasing concentration (or pressure for gases)
  • Increasing surface area of solids
• What is the relationship between temperature and the rate of reaction?

  Higher temperature increases the rate
• How does increasing concentration affect the rate of reaction?

  It increases the rate of reaction
• What is the effect of increasing pressure on the rate of reaction for gases?

  It increases the rate of reaction
• Why do reactions occur more quickly with increased energy during collisions?

  More particles collide with enough energy
• How do temperature and concentration affect the rate of reaction differently?

  Temperature affects energy; concentration affects frequency
• How does increasing temperature affect the rate of reaction?

  It increases the rate of reaction.
• What happens to the rate of reaction when concentration or pressure increases?

  • More particles in the same volume
  • More collisions occur
  • Reaction rate increases
• What does increasing the concentration of a solution do to the reaction rate?

  It makes collisions more likely.
• How does increasing pressure in a gas affect the reaction rate?

  It increases the frequency of collisions.
• How does breaking a solid reactant into smaller pieces affect the reaction rate?

  • Increases surface area to volume ratio
  • More area for particles to collide
  • Increases frequency of collisions
• Why does a larger surface area to volume ratio lead to a faster reaction rate?

  It allows more collisions to occur.
• What is the relationship between collisions and reaction rate?

  More collisions lead to a faster reaction.
• What is the implication of collision theory in reactions?

  Not every collision results in a reaction.
• What are the two factors affecting the rate of reaction in terms of collisions?

  1. Concentration (or pressure)
  2. Surface area of solid reactants
• What happens to the reaction rate when solid particles are smaller?

  The reaction rate increases.
• What is the effect of low concentration on reaction rate?

  It decreases the rate of reaction.
• What is the effect of high concentration on reaction rate?

  It increases the rate of reaction.
• What is the effect of low pressure on reaction rate?

  It decreases the rate of reaction.
• What is the effect of high pressure on reaction rate?

  It increases the rate of reaction.
• How does the size of solid particles affect the reaction rate?

  Smaller particles increase the reaction rate.