Rates of reaction

• Rate of reaction


  The speed at which the reactants change into products
• Ways to increase the rate of reaction

  • Increasing temperature
  • Increasing concentration
  • Decreasing the particle size/lump size
  • Adding a catalyst
• Increasing temperature


  • Particles move around more as they have more energy, meaning that they will bump into each other more at a faster speed causing more reactions
• Increasing concentration


  • There are more particles in the solution to move around which means there is a higher chance that they will collide, causing more reactions
• Decreasing particle size


  • More of the reactants are exposed to the other reactant which means that the reaction will be used up quicker
• Catalyst


  • Speeds up a reaction without being used up by the reaction, which means it can be extracted at the end of the reaction and be used again. This happens because the catalyst allows the reacting particles to collide with each other but with less energy so the reaction takes place at a lower temperature.
• Measuring mass and gas in a reaction

  1. Place the beaker the reaction is taking place on a scale to measure mass

  2. Use a gas syringe or a measuring cylinder filled with water to measure the volume of gas produced at regular time intervals
• Graphs

  • The line at the top is always the fastest reaction and the line at the bottom is always the slowest reaction
  • All reaction lines must be drawn so they meet at the same end point
  • There must be titles and the correct unit on the axis
  • If a 0 value is given, the graph must go through the origin
• Average rate of reaction

  The change in the quantity of chemical divided by the change in time