Equilibrium

Static equilibrium

Dynamic equilibrium

Enthalpy change

Reaction completion

It shifts the equilibrium position to the right to produce more products.

It shifts the equilibrium position to the left to produce more reactants.

It has no effect on the position of equilibrium.

It increases the equilibrium constant ($K_c$).

The system must be open to the surroundings.

The temperature must be continuously increasing.

The system must be closed.

The pressure must be kept at exactly 100 kPa.

If $Q < K$, the net reaction proceeds toward the reactants.

If $Q > K$, the net reaction proceeds toward the products.

If $Q = K$, the system is at equilibrium and no net change occurs.

If $Q = 0$, the system is already at equilibrium.

$2K_1$

$\frac{1}{K_1^2}$

$-2K_1$

$\sqrt{K_1}$

$K_c$ increases because the forward reaction is favored.

$K_c$ decreases because the reverse reaction is favored.

$K_c$ remains constant as it only depends on concentration.

$K_c$ remains constant but the yield of $SO_{3}$ decreases.