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Le Chatelier's Principle Lesson 2. If a system in equilibrium is stressed it shifts in the opposite direction to reach a new equilibrium . Chemists can shift the reaction to the Products or Reactants. Left. ⇌. reactants. products. - PowerPoint PPT Presentation
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Le Chatelier'sPrinciple
Lesson 2
What Happens in Vegas stays in Vegas
If a system in equilibrium is stressed it shifts in the opposite direction to reach a new equilibrium.
⇌reactants
products
Chemists can shift the reaction to the Products or Reactants
Left
If a system in equilibrium is stressed it shifts in the opposite direction to reach a new equilibrium.
⇌reactants
products
Chemists can shift the reaction to the Products or Reactants
Left
If a system in equilibrium is stressed it shifts in the opposite direction to reach a new equilibrium.
⇌reactants
products
Chemists can shift the reaction to the Products or Reactants
Right
If a system in equilibrium is stressed it shifts in the opposite direction to reach a new equilibrium.
⇌reactants
products
Chemists can shift the reaction to the Products or Reactants
Right
If a system in equilibrium is stressed it shifts in the opposite direction to reach a new equilibrium.
⇌reactants
products
Chemists can shift the reaction to the Products or Reactants
Right
If a system in equilibrium is stressed it shifts in the opposite direction to reach a new equilibrium.
⇌reactants
products
Chemists can shift the reaction to the Products or Reactants
Right
1.1 Increasing the temperature shifts in the direction that decreases energy:
A + B ⇌ C + Energy
stress- increase Temp reaction- shifts left
1.1 Increasing the temperature shifts in the direction that decreases energy:
A + B + Energy ⇌ C
stress- increase Temp reaction- shifts right
1.2 Decreasing the temperature shifts in the direction that increases energy.
A + B + Energy ⇌ C
stress- decrease Temp reaction- shifts left
2.1 Adding a reactant or product shifts the reaction in the direction that removes them.
A + B ⇌ C + Energy
reaction- shifts rightstress- increase [A]
2.2 Adding a reactant or product shifts in the direction that removes them.
A + B ⇌ C + Energy
stress- increase [C] reaction- shifts left
2.3 Removing a reactant or product shifts in the opposite direction.
A + B ⇌ C + Energy
stress- decrease [A] reaction- shifts left
2.4 Removing a reactant or product shifts in the opposite direction.
A + B ⇌ C + Energy
stress- decrease [C] reaction- shifts right
3.1 Only changes to (aq) and (g) reactants or products cause the equilibrium to shift
(s) and (l) have constant concentrations
You can change the concentrations of (aq) and (g)
CaCO3(s) + 2H+(aq) + 2Cl-
(aq) ⇌ Ca2+(aq) + Cl2 (g)
+ CO2(g) + H2O(l)
(s) and (l) do not!
no shift right left left leftright no shift
reactants
4.1 Adding a catalyst does not shift the equilibrium
Equilibrium is attained faster
Forward and reverse rates are increased by the same amount
products
5.1 Adding an inert (non-reactive) gas does not shift the equilibrium.
Adding Ne(g)
2NH3(g) ⇌ N2(g) + 3H2(g)
No shift!
The Forward and Reverse Rates and Shifting Explain in terms of the immediate changes to the forward and reverse rates after each stress why each shift occurs
2CO(g) + O2(g) ⇄ 2CO2(g) + energy
ShiftForwardReverse No change
IncreasesRight
1. Some CO is added- more reactant collisions.
The Forward and Reverse Rates and Shifting Explain in terms of the immediate changes to the forward and reverse rates after each stress why each shift occurs
2CO(g) + O2(g) ⇄ 2CO2(g) + energy
2. CO is removed. ShiftForwardReverse
leftdecreasessame
The Forward and Reverse Rates and Shifting Explain in terms of the immediate changes to the forward and reverse rates after each stress why each shift occurs
2CO(g) + O2(g) ⇄ 2CO2(g) + energy
3. Temperature is increased-
ShiftForwardReverse
increases increases by more
left
both forward and reverse rates increase.
We know it shifts left
