Equilibrium Constant in Gaseous Systems

In gaseous systems, the equilibrium constant, K_p​, represents the ratio of the partial pressures of products to the partial pressures of the reactants.

For a general reaction:

aA + bB ⇌ cC + dD

The equilibrium constant expression in terms of partial pressures (K_p​) is given by:

[Tex]K= \frac{[C]^c. [D]^d} {[A]^a. [B]^b}​[/Tex]

Where:

• [A], [B], [C], and [D] are the molar concentrations of the reactants and products at equilibrium,
• a, b, c, and d are the coefficients of the reactants and products in the balanced chemical equation.

The value of K_p​ depends only on the temperature and is constant at a given temperature. The value of Kp can be used to determine the nature of the reactants and products in the equilibrium reaction.

• If K​_p is much greater than 1, the products are favored at equilibrium.
• If K_p​ is much less than 1, the reactants are favored.
• If K_p​ is close to 1, equal amounts of both reactants and products are present at equilibrium.

Check, Applications of Equilibrium Constants

Equilibrium Constant K_p for a Few Selected Reactions

Equilibrium Constant K_p for a Few Selected Reactions is given in the table below:

Homogeneous Equilibrium is a state in a chemical reaction where all reactants and products are in the same phase. In this equilibrium, the rate of forward and backward reaction remains the same.

In this article, we will cover the basic ideas of homogeneous equilibrium, equilibrium constant, examples of homogeneous equilibrium along with a few problems based on the concept.