At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction, leading to no net change in the concentration of reactants and products over time.

At equilibrium, the concentrations of reactants and products remain constant over time, though they are not necessarily equal. The reaction continues at equal rates in both directions.

The equilibrium constant (K) is the ratio of the concentrations of products to reactants at equilibrium, each raised to the power of their stoichiometric coefficients.

If K > 1, the concentration of products is greater than that of reactants at equilibrium, indicating that the reaction favors the formation of products.

A catalyst speeds up the rate of both forward and reverse reactions equally, thus it does not affect the equilibrium position; it only helps the system reach equilibrium faster.

For an exothermic reaction, increasing temperature favors the reverse reaction (endothermic), shifting the equilibrium to the left to absorb the added heat.

Le Chatelier’s principle states that if a system at equilibrium is disturbed by a change in conditions, it will adjust to counteract the disturbance and restore equilibrium.

If the number of moles of reactants and products are equal in a balanced equation, the equilibrium constant (K) has no unit since the concentration terms cancel out.

Increasing pressure shifts the equilibrium towards the side with fewer moles of gas. If there are more moles of reactants, the equilibrium shifts to the left.

Dynamic equilibrium is characterized by the forward and reverse reactions occurring at the same rate, resulting in no net change in the system.