Define:
Reversible reaction
Products can react to form the original Reactants
What are some characteristics of Equilibrium Reactions?
- Closed system
no products or reactants escape - Concentration of reactants and products stays constant
- Dynamic
reactants and products are continuously reacting - Rate of forward reaction = Rate of reverse reaction
State:
Le Chatelier’s principle
If a disturbance is applied to a system in equilibrium,
Processes within the system will occur to counteract the change
What happens when you increase the concentration of reactants?
Equilibrium position will move to the right to favour forward reaction
More products are formed until equilibrium is restored
What happens when you increase the concentration of products?
Equilibrium position will move to the left to favour forward reaction
More reactants are formed until equilibrium is restored
For reversible equation: X(g) + Y(g) –> XY(g)
What happens if you increase the pressure of the system?
Equilibrium position will move to the right to favour forward reaction
Fewer gas molecules –> less pressure
When increasing pressure, do you take into account the number of moles of solids/liquids to find the equilibrium position?
NO
molecules/ions in solids/liquids are densely packed together –> can’t be compressed easily
