Chemistry

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  • Chemistry
    • Collision theory
      • Reaction rates are explained by collision theory.
        • The rate of a reaction depends on how often and how hard the reacting particles collide with each other.
          • More collisions increase the rate of reaction
      • Higher temperature increases collisions
        • When the temperature is increased the particles all move quicker. If they are moving quicker they are going to collide more.
      • Higher concentraion (or pressure) increases collisions
        • In a gas, increasing the pressure means the particles are more asquashed up together so there will be more frequent collisions
      • Larger surface area increases collisions
        • If one of the reactants is a solid then breaking it up into smaller pieces will increase the total surface area. This means the particles around it in the solution will have more area to work on, so there'll be more frequent collisions.
    • Increasing the temperature causes faster collisions
      • Reactions only happen if the particles collide with enough energy
        • The minimum amount of energy needed by the particles to react is known as the activation energy
          • At a higher temperature there will be more particles colliding with enough energy to make the reaction happen
    • Catalysts
      • Many reactions can be speeded up using a catalyst
      • A catalyst is a substance which speeds up a reaction, without being changed or used up in the reaction.
  • The rate of a reaction depends on how often and how hard the reacting particles collide with each other.
    • More collisions increase the rate of reaction

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