Reversible Reactions
- 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
- many reactions have a greater volume on one side (either)
- "a reversible reaction is one where the PRODUCTS can react themselves to produce the ORIGINAL REACTANTS"
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