Question

What is meant by nitrogen fixation? Describe a process for fixation of nitrogen on an industrial scale.

Short answer

Nitrogen fixation makes atmospheric nitrogen usable by plants. The Haber-Bosch process industrially fixes nitrogen into ammonia using nitrogen and hydrogen gases.

Step-by-step solution

Understanding Nitrogen Fixation

Nitrogen fixation refers to the process of converting nitrogen gas (N₂) from the atmosphere into ammonia (NH₃) or related nitrogenous compounds in soil, which plants can then absorb and use for growth. This is an essential natural process that makes nitrogen accessible to living organisms, as atmospheric nitrogen is not in a form that plants can use directly.

Introducing the Haber-Bosch Process

On an industrial scale, the Haber-Bosch process is the primary method used for the fixation of nitrogen. This process synthesizes ammonia from nitrogen and hydrogen gases under high temperature and pressure, in the presence of an iron or ruthenium catalyst.

Understanding the Reaction Condition

The chemical reaction for the Haber-Bosch process is: \[ N₂(g) + 3H₂(g) ightarrow 2NH₃(g) \]This reaction occurs at a temperature of about 400-500°C and a pressure of 150-200 atmospheres. These conditions favor the formation of ammonia according to the principles of chemical equilibrium and kinetics.

Importance of the Haber-Bosch Process

The ammonia produced through the Haber-Bosch process is mainly used to produce fertilizers, which are crucial in supporting global agriculture. This process enables human ability to grow enough food to feed billions of people by supplementing natural nitrogen fixation processes.

Key concepts

Haber-Bosch process

The Haber-Bosch process is a groundbreaking industrial procedure that revolutionized agriculture and industry. It enables the direct synthesis of ammonia (\( NH_3 \)) from atmospheric nitrogen (\( N_2 \)) and hydrogen (\( H_2 \)) gases. This method was a significant scientific breakthrough, developed by Fritz Haber and Carl Bosch in the early 20th century. The process operates under rigorous conditions:

• High temperature: approximately 400-500°C
• High pressure: around 150-200 atmospheres
• Use of catalysts: usually iron or ruthenium to speed up the reaction

These specific conditions push the nitrogen and hydrogen to react and form ammonia, which wasn't easily achievable before the development of this process. Additionally, through careful management of reaction conditions, industries can maximize the yield of ammonia, essential for many applications, particularly in producing fertilizers. This advancement has been pivotal in boosting food production globally, allowing for more consistent agricultural productivity.

ammonia synthesis

Ammonia synthesis is the chemical process where nitrogen gas (\( N_2 \)) and hydrogen gas (\( H_2 \)) react to form ammonia (\( NH_3 \)). This reaction may seem simple, but it requires precise conditions to be feasible on an industrial scale:

• Reaction Equation: \[ N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) \]
• High-energy barriers: The strong triple bond in nitrogen molecules (\( N\equiv N \)) makes the reaction challenging without high heat and pressure.
• Activated Catalysts: Catalysts such as iron or ruthenium are essential for lowering these energy barriers, making the nitrogen and hydrogen atoms easier to combine.

Ammonia synthesis is central to industrial chemistry because of its vast application in producing fertilizers and other chemicals. It also highlights the role of "chemical engineering" in optimizing conditions to enhance efficiency and economic viability. By effectively synthesizing ammonia, industries can produce essential compounds for various uses, driving both economic and agricultural development worldwide.

industrial nitrogen fixation

Industrial nitrogen fixation is the conversion of atmospheric nitrogen (\( N_2 \)) into usable forms of nitrogen like ammonia (\( NH_3 \)) on a large scale. This process is crucial because, although nitrogen makes up a significant portion of Earth's atmosphere, it is not directly accessible to most living organisms due to its unreactive nature. The Haber-Bosch process is a prime example of industrial nitrogen fixation:

• Transformative Impact: It allows the production of fertilizers necessary to support agricultural needs.
• Economic Significance: By producing ammonia efficiently, it lowers costs in fertilizer production, benefiting global agriculture and economies.
• Environmental Considerations: While essential, the process requires significant energy and contributes to greenhouse gases, prompting ongoing research into more sustainable practices.

Understanding industrial nitrogen fixation through the Haber-Bosch process demonstrates the interplay between chemistry and industry. It illustrates the need for balancing technological advancement with environmental stewardship, ensuring the availability of resources for future generations.