Question

What is a homogeneous reaction? What is a heterogeneous reaction? Give examples.

Short answer

A homogeneous reaction is one in which all reactants and products are in the same phase, like the formation of ammonia in the Haber process. A heterogeneous reaction involves reactants and products in different phases, such as the reaction of calcium carbonate with hydrochloric acid to form carbon dioxide.

Step-by-step solution

Define a Homogeneous Reaction

Identify the characteristic of a homogeneous reaction. It is a reaction where all the reactants and products are in the same phase. An example is the reaction of nitrogen and hydrogen gases to form ammonia gas in the Haber process: \[ N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) \]

Define a Heterogeneous Reaction

Describe what a heterogeneous reaction entails. This reaction occurs when the reactants and products are in different phases. A common example is the reaction between a solid and a gas, such as the formation of carbon dioxide when calcium carbonate (solid) reacts with hydrochloric acid (aqueous): \[ CaCO_3(s) + 2HCl(aq) \rightarrow CaCl_2(aq) + H_2O(l) + CO_2(g) \]

Key concepts

Homogeneous Reaction

A homogeneous reaction refers to a chemical process where all the reactants and products are in a single phase, whether solid, liquid, or gas. This uniformity ensures that the substance's composition is consistent throughout, causing the reactants to interact with each other more efficiently due to the absence of phase boundaries.

For instance, when nitrogen (N_2) gas reacts with hydrogen (H_2) gas under certain conditions, they form ammonia (NH_3) gas. This reaction can be represented by the equation: \[ N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) \]
Here, the '(g)' notation signifies that all involved substances are in the gaseous phase, making the reaction homogeneous. Homogeneous reactions are often observed in solutions where solutes are dissolved in a solvent to form a single, uniform phase.

Heterogeneous Reaction

On the other hand, a heterogeneous reaction occurs when the participating substances exist in two or more different phases. The interfaces between these phases can sometimes hinder the reaction rate due to limited contact between reactants.

A classic example involves a solid reactant interacting with a liquid or gaseous reactant, such as the reaction of calcium carbonate (CaCO_3), a solid, with hydrochloric acid (HCl), an aqueous solution, to yield calcium chloride (CaCl_2) in aqueous form, water (H_2O) as a liquid, and carbon dioxide (CO_2) gas:\[ CaCO_3(s) + 2HCl(aq) \rightarrow CaCl_2(aq) + H_2O(l) + CO_2(g) \]
This equation clearly shows the involvement of different phases: '(s)' for solid, '(aq)' for aqueous, and '(g)' for gas, characterizing the reaction as heterogeneous.

Haber Process

The Haber process, a critical method for producing ammonia, is an example of a homogeneous reaction involving gases. This industrial process synthesizes ammonia from nitrogen and hydrogen gases, using an iron catalyst under high temperature and pressure conditions:

\[ N_2(g) + 3H_2(g) \leftrightarrow 2NH_3(g) \]
The reaction is reversible and reaches a dynamic equilibrium, meaning the rates of the forward and reverse reactions are equal. This process represents a major breakthrough in chemistry as it enables the large-scale production of ammonia for fertilizers, which in turn supports global agriculture.

Reaction Phases

Reaction phases refer to the distinct physical states - solids ((s)), liquids ((l)), aqueous solutions ((aq)), and gases ((g)) - that can be involved in a chemical reaction. The phase of a substance significantly influences the rate and mechanism of the reaction. Homogeneous reactions take place within a single phase, facilitating quick and uniform mixing of reactants, whereas heterogeneous reactions involve reactants in different phases, which may affect the contact between them and influence the reaction dynamics.

Understanding the phases of reactants is crucial for predicting the behavior of reactions and for designing processes such as the Haber process, which relies on maintaining a gaseous phase to produce ammonia efficiently.