Reversible Reactions

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  • Created by: Jo Wells
  • Created on: 18-04-13 20:48
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  • Reversible Reactions
    • "a reversible reaction is one where the PRODUCTS can react themselves to produce the ORIGINAL REACTANTS"
      • A+B <--> C+D
    • equilibrium
      • (if takes place in a closed system - nothing else effecting it)
      • means the amounts of reactants and products will reach a certain balance and stay there
        • reactions are still happening both directions, but they cancel each other out
      • if you deliberately alter the temperature/ pressure you can move the 'position of equilibrium' - give more product & less reactants
        • adding a catalyst doesn't change the equilibrium position - merely speeds the rate up
      • adding a catalyst doesn't change the equilibrium position - merely speeds the rate up
    • changing temperature
      • all reactions are exothermic one way and endothermic the other way
      • if you INCREASE the temperature the ENDOTHERMIC reaction will use up the extra heat
        • increasing the endothermic reaction
      • if you DECREASE the temperature the EXOTHERMIC reaction will give out more heat
        • increasing the exothermic reaction
    • changing pressure
      • many reactions have a greater volume on one side (either)
        • greater volume means more gas molecules and less volume = fewer gas molecules
      • if you INCREASE the pressure it will increase the side with LESS volume
      • if you DECREASE the pressure it will increase the side with MORE volume

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