rates of reaction

    Cards (15)

    • collision theory 

      for a successful collision molecules have to collide with sufficient energy and must collide in correct orientation
    • activation energy
      minimum amount of energy to start a reaction
    • concentration of solution
      higher the concentration the faster the reaction
      particles are now closer together so more frequent successful collisions
    • surface area of a solid
      the more surface area the faster the rate of reaction
      more particles are exposed for particles to collide leading to more successful collisions
    • pressure of gases 

      the more pressure the faster the rate of reaction
      less space for molecules to move around cause them to collide leading to more successful collisions
    • temperature
      the higher the temperature the faster the rate of reaction
      temperature increases the movement of particles due to more kinetic energy cause particles to collide more leading to more successful collisions
    • catalyst
      if there is a catalyst the rate of reaction is faster
      this is because it lowers the activation energy and provides a alternative pathway leading to particles to collide more
    • catalyst
      substance that speeds up reaction without being used up by lowering activation energy by providing an alternative pathway
    • desorbed means leaving the substance
    • absorbed means through the whole substance
    • adsorbed means only on the surface
    • catalysts: how do they work?

      substance is adsorbed on surface of catalyst near active site
      weakening bonds/more favourable orientation
      reaction taking place
      products are desorbed
    • homogenous
      reactants and catalyst are in the same state
    • heterogenous
      reactants and catalysts are at different states
    • catalytic converters are heterogenous