Rates of Reaction

• more collisions = greater rate of reaction
• For a reaction to happen:

  reactant particles MUST collide with eachother with enough energy
• Activation energy =

  the minimum amount of energy required for a reaction to happen
• There are 3 things that affect the rate of reaction. They are:

  temperature, concentration and surface area
• A fast reaction (like combustion) happens in a short time
• A slow reaction (like rusting) happens over a long time
• More particles in the same volume results in more successful collisions, so rate of reaction increases
• A higher temperature results in a faster rate of reaction because the particles gain more energy and moves faster, resulting in more frequent collisions
• If there are more particles of reactant available:

  there is an increase in frequency of successful collisions
• Catalysts provide an alternative reaction pathway with a lower activation energy
• Successful collisions:

  A collision between reactant particles that has enough energy for a reaction to happen.