which makes up for the
which is illustrated in
as the reverse reaction collisions form reactants
therefore within the favored forward reaction
(products >) resulting in a greater reverse rate of reaction for the
greater forward rate of reaction (reactants>) increases the
where a higher concentration of reactants/products particles results in
which is the shift to increase the
at particle level can be explained through
until new equilibrium position is reached; predicted as
the equilibrium shift favors of system's
results in a value Q< K where the
which counteracts and makes up for the
this system shift therefore increases
until new equilibrium position is reached
then equilibrium shift will favour the system's
resulting in a value Q>K
which can occur through the chemical system's
which can occur within the system by
can be affected by the chemical system's
K magnitude indicates the
which is defined by the
which describe the chemical system (at equilibrium) mathematically through
which observes that a chemical system will adjust to
through predictable shifts, as stated in
as the result of specific changes in
which occurs in order to restore the
cause a chemical system to
therefore the position of equilibrium opposes the
equilibrium at particle level explained by the

Concentration Changes

Shift Equilibrium

Equilibrium State

Chatelier's Principle

Oppose (Minimize) Stresses on Chemical System Equilibrium

Reactant and Product Concentrations

Equilibrium Law

Equilibrium Law Constant

c1

Position of the Equilibrium

Change Concentration of Entities in Equilibrium

Increase in [Products]/ Decrease in [Reactants]

Reactants < Products

Reverse Reaction (Reduce [Product])

Reactants Form as Products Concentration Decrease

Reactant Production ↽

[Reactant] Decrease

Increase in Reactants/Decrease in Products Concentration

Reactants > Products

Forward Reaction (Reduce [Reactant])

Products Concentration Increase as Reactants Concentration Decrease

Collision Theory

Increase Particle Collision Frequency (Probability of Successful Collisions)

Formation (Concentration) of Products

[Reactants] must be Used Up

Decomposition into Reactants

[Products] must be Used Up

Equilibrium Graphs

Product Production ⇀

[Product] Decrease