Reaction Rate and Collision Theory

• COLLISION THEORY

  Collison theory states that for a chemical reaction to occur, the reacting particles must collide with one another with enough activation energy and in proper orientation
• COLLISION THEORY

  The rate of reaction depends on the frequency of collisions
• CONCENTRATION

  • If there is more of a substance in a system, there is greater chance that molecules will collide and speed up the rate of the reaction

  If there is less of something, there will be fewer collisions and the reaction will probably happen at slower speed

  
• CONCENTRATION

  A) low

  B) greater

  
• TEMPERATURE


  The higher the temperature, the higher is the kinetic energy possessed by the reacting particles which causes them to move faster. Essentially, the greater is their chance of collision, and the faster is the reaction.

  
• PARTICLE SIZE


  The smaller the particle size of the reactant, the more exposed are its surfaces to the other reactant and therefore the greater is the chance of reaction to occur faster.

  
• NATURE OF REACTANTS


  The rate of a reaction depends on the nature of the reactants.

  The rate of reaction is faster in case of a more reactive metal than a less reactive metal

  
• NATURE OF REACTANTS

  For example, the active metals calcium and sodium both react with water to form hydrogen gas and a metal hydroxide. However, calcium reacts moderately, while sodium reacts almost explosively and rapidly. This is so because sodium is more reactive than calcium.
• Catalyst speeds up reaction but it is not used up in the reaction
• Catalytic Reaction

  A) Energy

  B) Reaction

  C) Catalyzed reaction

  D) Uncatalyzed reaction

  
• APPLICATION OF CATALYST IN EVERYDAY LIFE

  • HABER PROCESS – to produce ammonia for fertilizer
  • CONTACT PROCESS – to produce sulfuric acid for detergent and fertilizer
  • CATALYTIC CONVERTER