Factors that affect the rate of chemical reaction

• Collision theory - For particles to react, they have to collide with each other with sufficient activation energy (or activation energy) if particles collide with less energy than the activation energy then nothing will happen.
• 1. Amount of energy the particles have - more energy they have, the more energy can transferred during the collision and the more likely they are to surpass the minimum activation energy.
• 2. Frequency of collision - How often the particles collide with each ther. Not all collisions are successful because the particles involved don't always reach th activation energy.
• More often they collide ---> more successful collisions overall
• Factors:

  Temperature

  Concentration/pressure

  catalyst

  surface area
• Catalysts speed up reactions by providing an alternative pathway which has a lower activation energy compared to the normal one. This allows more frequent successful collisions to occur, leading to an increased rate of reaction.

  
• Surface area is important as it increases the number of successful collisions between molecules. The greater the surface area, the more chance there is for particles to collide successfully.
• Increasing temperature causes kinetic energy to increase so particles move faster and collide more frequently. More collisions means more successful ones too. Increased frequency of successful collisions leads to higher rates of reaction.
• The concentration of reactants affects the rate of reaction. As the concentration increases, the likelihood of successful collisions also increases due to the fact that there are more particles present.
• When pressure or concentration increases, the rate of reaction increases because there are more particles available for collision.
• Activation energy is the minimum energy required to cause a process (such as a chemical reaction) to occur.