Homogeneous And Heterogeneous Equilibrium

We see a variety of reactions in our everyday lives, such as iron rusting, paper burning, curd sourness, ozone formation, and so on. Many of these reactions necessitate the existence of components in different phases, such as solid iron combining with gaseous oxygen to produce solid iron oxide, often known as rust. Similarly, liquid water is formed when gaseous hydrogen and oxygen mix. Dealing with such responses is a time-consuming task. When the components are in the same phase, their interaction is straightforward; but, when the components are in various stages, the interaction becomes more difficult to comprehend.

Equilibrium

It  is a state of chemical reaction in which the forward and backward reaction rates are equal. In addition, there are two types of equilibrium: homogeneous and heterogeneous equilibrium. A homogeneous mixture is a homogeneous equilibrium in one phase (reactants and products in a single solution). Remember that the reactants are on the left and the products are on the right side of the equation. As a result, the solute response corresponds to a single homogeneous equilibrium. A reactive system with a heterogeneous equilibrium, on the other hand, has products and reactants in two or more phases.

Homogeneous Equilibrium

Equilibrium is a state of chemical reaction in which the rates of backward and forward reactions are equal. In addition, there are two types of equilibrium: heterogeneous and homogeneous equilibrium. A homogeneous mixture (products and reactants in a single solution) is a homogeneous equilibrium in one phase. Keep in mind that the reactants are on the left side of the equation, while the products are on the right. As a result, the reaction between the solutes is contained inside a single homogeneous equilibrium. On the other hand, a heterogeneous equilibrium is a chemical system in which the reactants and products are dispersed throughout two or more phases.

Example of Homogeneous Equilibrium

There are two different types of homogeneous equilibrium. In the first category, the number of molecules in the product is the same as the number of molecules in the reactants of that particular equation.

N2 (g) + O2 (g)→ 2NO, for example (g)

On the right side of the diagram, we can see two molecules of reactants (one of each) and two molecules of product. In the second category of a homogeneous equilibrium equation, the opposite events occur. The number of molecules in the product is not the same as or equal to the number of molecules in the reactant.

Consider the following scenario:

2SO3 →2SO2 (g) + O2 (g) (g)

We can see from the preceding example that the reaction only has three reactant molecules and two product molecules

Heterogeneous Equilibrium

The system is homogeneous equilibrium when the products and reactants of an equilibrium reaction form a single phase, whether gas or liquid. The concentrations of the reactants and products might vary greatly in such scenarios. A heterogeneous equilibrium, on the other hand, is a system in which the reactants, products, or both are in more than one phase, such as the reaction of a gas with a solid or liquid.

Difference between Homogeneous and Heterogeneous Equilibrium

The term “equilibrium” refers to a state in which the concentrations of reactants and products remain constant. The two forms of equilibria are homogeneous and heterogeneous equilibrium. In homogeneous equilibrium, the reactants and products are in the same phase of matter, whereas in heterogeneous equilibrium, they are in different phases of matter.

Furthermore, we must include the concentrations of all reactants and products when determining the equilibrium constant for homogeneous equilibria; however, when determining the equilibrium constant for heterogeneous equilibria, we must exclude the concentrations of solids and pure liquids and use the concentrations of other reactants and products. As an example, a homogeneous equilibrium is 2SO2(g) → O2(g) 2SO3(g),

while a heterogeneous equilibrium is O2(g) + 2C(s) →2CO(g).

To put it another way, equilibrium is when the concentrations of reactants and products are constant. The two forms of equilibria are homogeneous and heterogeneous equilibrium. In homogeneous equilibrium, the reactants and products are in the same phase of matter, whereas in heterogeneous equilibrium, they are in different phases of matter. Furthermore, for homogeneous equilibria, the equilibrium constant includes all reactant and product concentrations, whereas for heterogeneous equilibria, solid and pure liquid concentrations must be excluded.

Conclusion

As we conclude from above, a homogeneous equilibrium is one in which the products and reactants are in the same phase; a heterogeneous equilibrium is one in which the reactants, products, or both are in different phases.