Temperature

• Collision Theory


  Chemical reactions can only take place when the reacting particles collide with each other, and the collisions must have sufficient energy
• Reaction rate


  Determined by the frequency of successful collisions (number of collisions per second)
• Activation energy


  The minimum amount of energy that the particles must have in order to react (collide successfully)
• Particles with low energy collide


  Cannot overcome activation energy barrier, no reaction occurs
• Particles with high energy collide

  Can overcome activation energy barrier, reaction occurs
• Increasing temperature


  Increases the energy of the particles, making them move faster
• Increased particle energy and movement


  Increases the frequency of collisions (more collisions per second)
• Increased particle energy


  More particles can overcome activation energy barrier and collide successfully
• Increasing temperature


  Increases the rate of chemical reaction
• The rate of reaction is proportional to the temperature
• Collision Theory


  Chemical reactions can only take place when the reacting particles collide with each other and the collisions must have sufficient energy
• Rate of reaction


  Determined by the frequency of successful collisions (number of collisions per second)
• Activation energy


  The minimum amount of energy that the particles must have in order to react (collide successfully)
• Particles with low energy collide

  Cannot overcome activation energy barrier, no reaction occurs
• Particles with high energy collide

  Can overcome activation energy barrier, reaction occurs
• Increasing temperature


  Increases the rate of chemical reactions
• Why increasing temperature increases reaction rate

  • Increases the energy of the particles, causing them to move faster and increasing the frequency of collisions
  • Increases the number of particles that can overcome the activation energy barrier and collide successfully
• The rate of reaction is proportional to the temperature