Chemical Equilibrium
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Le Châtelier’s Principle
Chemical system I. Dynamic equilibrium will remain in equilibrium indefinitely until acted upon by an outside influence
Concentration
Changing the concentration of a reactant or product that appears in the equilibrium expression temporarily knocks the system out of equilibrium; the system then responds accordingly to move back to equilibrium
Increasing [reactant] or decreasing [product]:
Shifts the system to the right
Decreasing [reactant] or increasing [product]:
Shifts the system to the left
Pressure
Changing the external P on a system at equilibrium by changing the V of the rxn container temp. Knocks the system out of equilibrium only if the balanced rxn has different #s of gas molecules in the reactant and product sides
Increasing external P:
Shifts the system toward the side with fewer gas molecules
Decreasing external P:
Shifts the system toward the side with more gas molecules
Temperature
Changing T always changes the position of equilibrium; does not knock out of equilibrium but moves the actual position of equilibrium because all K’s are T dependent
The only way of changing the value of the equilibrium constant
Is to change T
Q>K
The system has too much product and must therefore shift to the left to reach equilibrium
Q
The system has too much reactant and must shift to the right to reach equilibrium
Q=K
In equilibrium and should really be using K instead of Q