Le Chatelier's Principle

Temperature

Pressure

Catalyst

Concentration

The equilibrium will shift to the right.

The equilibrium will shift to the left.

The equilibrium will remain unchanged.

The reaction will stop.

Shift to the right

Shift to the left

No change

Reaction stops

Because it increases the concentration of reactants.

Because it decreases the concentration of products.

Because it favors the endothermic reverse reaction.

Because it increases the rate of the forward reaction.

The equilibrium will shift to the right.

The equilibrium will shift to the left.

The equilibrium will remain unchanged.

The reaction will stop.

$$K_c = \frac{[H_2][I_2]}{[HI]^2}$$

$$K_c = \frac{[HI]^2}{[H_2][I_2]}$$

$$K_c = [H_2][I_2]$$

$$K_c = [HI]^2$$

Increases the rate of reaction and shifts equilibrium to the right.

Increases the rate of reaction but does not affect the position of equilibrium.

Decreases the rate of reaction and shifts equilibrium to the left.

Decreases the rate of reaction but does not affect the position of equilibrium.

The equilibrium will shift to the right.

The equilibrium will shift to the left.

The equilibrium will remain unchanged.

The reaction will stop.

It changes with concentration.

It changes with temperature.

It changes with pressure.

It changes with the presence of a catalyst.

The equilibrium will shift to the right.

The equilibrium will shift to the left.

The equilibrium will remain unchanged.

The reaction will stop.