Equilibrium Flashcards
Equilibrium State
Rate of forward reaction = rate of backwards reaction
Dynamic in nature (even though it looks like the reaction has stopped it hasn’t)
The concentrations of all reactants and products remain a constant
Temperature dependent
Properties of K
Unitless
Temperature dependent
Constant for a given reaction
Higher K = more products, equilibrium more to right
Lower K = More reactants, equilibrium position is more to the left.
What happens to K when reverse reaction?
1/K
What happens to K when reaction is multiplied by a number?
K^n
What happens to K when reaction is divided by a number?
K^1/n
What happens to K when reactions are added?
K*K
Q
Reaction is still going forward to reach equilibrium
Q = K
Reaction is at equilibrium
Q > K
Reaction has to go backwards to regain equilibrium
Le Chatelilier’s Principle
If a constant is applied to a system at equilibrium, the system will readjust the equilibrium position so as to minimize the effect of the constraint.
How does changing the concentration change equilibrium?
Wherever there is less, the reaction will move to that side.
Ways to change Pressure
Changing Volume
Adding inert gas
Change in Temperature
How does changing the volume change equilibrium?
Decrease in Volume = shifts to wherever there is less mols
Increase in Volume = shifts to wherever there is more mols
How does adding an inert gas change equilibrium?
No change in equilibrium position, as it only changes the total pressure but not the individual pressures.
How does changing the temperature in an exothermic reaction change equilibrium?
H = - , heat on right
Increasing temperature means the system wants to decrease temperature, it will shift equilibrium to left, opposite for decreasing temperature
