| What does Le Chatelier's Principle say? | -This is simply saying that a Change in either: Concentration, Pressure or Temperature will have the Equilibrium Position move to Fight that Change
-Can ONLY happen in a Reversible Reaction |
| How can Temperature affect the Position of Equilibrium | -The Position of Equilibrium will be Affected by Temperature because either the Forward will be Exothermic or Endothermic, and the Backwards would be Opposite to the Forward
-Decreasing the Temperature means the Position of Equilibrium will move in the Exothermic Direction, to Make more Heat
-Increasing the Temperature means the Position of Equilibrium will move in the Endothermic Direction, to Absorb more Heat |
| Example: N₂ + 3H₂ ⇌ 2NH₃
-If the Forward Reaction is Exothermic, then what will happen to the Position of Equilibrium if the Temperature Decreased? | -If the Temperature Decreases, then the Position of Equilibrium will move to Counter that Change, by shifting towards the Exothermic Reaction, so more 2NH₃ is Made [Product] |
| How can Pressure affect the Position of Equilibrium? | -Increasing the Pressure will have the Position of Equilibrium move towards the Side with the Least Amount of Moles, this Reduces Pressure
-Lowering the Pressure will have the Position of Equilibrium move towards the Side with the Most Amount of Moles. This Increases Pressure |
| Example N₂ + 3H₂ ⇌ 2NH₃
-What happens if the Pressure Increased? | -Since the Pressure Increased, the Position of Equilibrium will move in a way to Counter that Change, so it will move with the Side that has the Least Amount of Moles, and that being 2NH₃ [2 Moles to 4 Moles] |
| How can the Concentration affect the Position of Equilibrium? | -Increasing the Concentration of Reactants will want the Position of Equilibrium to Lower that, so it will go Towards the Products Side, using More of it Up
-Increasing the Concentration of Products will want the Position of Equilibrium to Lower that, so it will go Towards the Reactants Side, using More of it Up |
| Example N₂ + 3H₂ ⇌ 2NH₃
-What happens if the Concentration of the Reactants Increased? | -Since the Concentration has been Increased, the Position of Equilibrium will move in a way that Counters that Change -It will use up more Reactants
-So therefore the Position of Equilibrium will move Left |
