chp 11

• forward reaction

  if equilibrium shifts so the forward reaction is favoured (reactants - products) we say equilibrium shifts to the right (more products are made)
• backwards reaction


  if equilibrium shifts so the backwards reaction is favoured (products - reactants) we say equilibrium shifts to the left (more reactants are made)
• exothermic

  more reactants, less products

  activation energy = difference between top and reactants level

  energy released = difference between reactants and products

  change is negative
• endothermic

  less reactants, more products

  activation energy = difference between top and reactants level

  energy absorbed = different between reactants and products

  change is positive
• maxwell blotzmann

  when you add the catalyst you need less energy required for the reaction to happen than if you don't have it

  when you use a catalyst it also speeds up the reaction as the particles themselves don't need as high of activation energy