Rate of reaction

• The rate of reaction is defined as the the change on concentration of a reactant or pdouct per unit of time.
• Collision theory states that a reaction owuld occur when particles collide with sufficient energy and in the correct orentiation. This is known as activation energy and when the energy is absorbed they undergo a transition state which is the maximum potential energy of the reaction.
• The rate of reaction increases as the frequency of collisions increases, this is achieved through increasing

  1. Surface area
  2. Pressure
  3. concentration
  4. Temperature
• Maxwell-Boltzmen states that the particles in a substance have a range of kinect energy during a reaction, this is indicated with the shaded area under the graph
• Catalyst is a substance that speeds up the reaction by providing an alternative energy pathway that lowers the activation energy
• Homogenous state is when the reactants and products are in the same state, while hetergenous is when they are not