Topic 7

• The minimum amount of energy that particles must collide with to react.

  Activation Energy
• Chemical reactions only occur when colliding particles colldie with the correct orientation and with suffice to energy.

  Collision Theory
• Increasing the concentration of reactants means the reacting particles will be closer together, meaning they will collide more often.

  Effect of Concentration on Reaction Rate
• Increasing the pressure of gaseous reactant means the reacting particles will be closer together, meaning they will collide more often.

  Effect of Pressure on Reaction Rate
• Increasing the surface area of the reactants means there are more exposed reacting particles, meaning there are more frequent successful collisions.

  Effect of Surface Area on Reaction Rate
• Increasing the temperature means the particles will have more kinetic energy ans so will move faster, colliding more often and a larger proportion of the particles will have enough for activation energy.

  Effect of Temperature on Reaction Rate
• Biological catalysts which speed up biochemical reactions so that organisms can survive. They are used in the production of alcoholic drinks.

  Enzymes
• The reaction in which an acid and a base react together to form salt and water.

  Neutralisation
• The difference between the sum of the energy needed to break bonds in the reactants and the sum of the energy released when bonds in the products are formed.

  Overall Energy Change of the Reaction
• A reaction in which solutions react to form an insoluble product.

  Precipitation Reaction
• The measure of the amount of product formed or reactant used over time. The units can be given as g/s, cm^3/s or mol/s.

  Rate of Reaction
• Graphs used to show the relative energies of reactants and products, the activation energy and the overall energy change of a reaction.

  Reaction Profile