Collision Theory
Updated: 5/27/2020
Collision Theory
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Storyboard Text

  • Reactions can only happens when particles collide, but not all end up in a reaction. Many particles bump off each other instead.
  • What does the collision theory state?
  • The collision theory states, the reactant particles must collide with each other and the collision needs to have sufficient energy in order for a reaction to occur.
  • In order for a reaction to happen, activation energy is needed.
  • Activation energy is the minimum amount of energy needed for particles collide successfully.
  • What is Activation Energy?
  • This is a diagram of the reaction between calcium carbonate and hydrochloric acid.
  • Only the particles on the surface are available for collisions. The frequency of successful collisions increases as the surface area of the solid increases.
  • What is a successful collision?
  • Successful collisions are collisions with energy greater than or equal to the activation energy.
  • Changing the temperature of the reaction causes the reaction to speed up or slow down depending on whether the temperature is increased or decreased.
  • Increasing the pressure of the reaction, makes no difference to the rate of reaction if it is a solid or liquid. However, increasing the pressure in a gas speeds up the reaction. The forces the particles closes together, so the collide more frequently. This is exactly the same as increasing the concentration of the gas.
  • Concentration of ReactantsReducing the concentration of the acid, makes the reaction slower.
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