Collision Theory

• • For a reaction to happen the reacting particles must successfully collide.
• • A successful collision happens when the reacting particles have sufficient energy.
• Collision theory

  
• • Rate of reaction depends on the frequency of successful collisions between the reacting particles, so the greater the frequency of the successful collisions, the faster the rate or reaction.
• Energy profile diagram

  
• • The activation energy is the minimum energy required for a collision to be successful - It’s the quantity of energy required to get the reaction started.
• • Collisions that have the required activation energy are successful in producing a reaction - collisions with insufficient energy don’t produce a reaction.
• • Increasing the rate of reaction increases the chance / frequency of successful collision.
• There are four ways if changing the rate of reaction:

  • Temperature
  • Concentration
  • Surface area
  • Catalyst