Rates Of Reaction

• Factors Affecting Rates of Reaction


  Bullet points: Concentration, Temperature, Surface Area, Catalysts
• Activation Energy


  The minimum energy required for a reaction to occur
• Effective Collisions


  Reactant molecules collide with sufficient energy and proper orientation, resulting in a reaction
• Increasing surface area increases reaction rate by providing more


  area for reaction to occur and collisions become more frequent
• Increased temperature


  Increases kinetic energy, increases frequency of collisions, increases rate of reaction
• Concentration doubles


  Rate of reaction doubles
• Catalyst added

  Reaction rate increases, decreases amount of activation energy needed by finding an alternative pathway with a lower activation energy amount.
• The conditions for a reaction to occur according to collision theory are:

  Particle frequency, the more collisions the faster the reaction is. Particle energy, particles have to collide with enough energy for the reaction to be successful.
• Equilibrium


  A state where the rates of forward and reverse reactions are equal.
• Le Chatelier's Principle


  A principle that states that systems in equilibrium will respond to changes by shifting the equilibrium to counteract the change by favouring either the forward or reverse reaction.