Haber-Process of Ammonia
In Haber Process of Ammonia, methane and water undergo reactions internally to generate hydrogen. Later, oxygen and nitrogen gas are introduced, initiating another process that generates additional hydrogen from methane. In both reactions, carbon monoxide forms as a by-product.
The components of ammonia N2 and H2 combine in a ratio of 1:3.
N2(g) + 3H2(g) ⇌ 2NH3(g) with ΔH = −92.4kJ/mol
After that water vapor is introduced, leading to the oxidation of carbon monoxide to carbon dioxide. The produced carbon dioxide exits the system, leaving behind a gas mixture of nitrogen and hydrogen. This mixture undergoes compression at 200 atmospheres and is heated at approximately 500°C. The heated and pressurized mixture then enters the reaction chamber and then put a metal catalyst (Iron) with small amounts of K2O and Al2O3 to increase the rate of attainment of equilibrium. Ammonia is formed in this stage, and the reaction mixture is distilled by passing a cold water jacket over it. This ammonia gas goes for liquefaction, which is drained from the system.
Initially, only around 15% of the nitrogen and hydrogen undergo reaction. The unreacted gas separates from the liquid ammonia and goes back to the reaction chamber. Through further runs, approximately 98% of the original gas mixture eventually reacts to produce ammonia.
Haber’s Process
Haber’s Process, which is also called the Haber-Bosch process, is used in the synthesis of ammonia from nitrogen and hydrogen. The Haber process to produce ammonia was developed during World War 1 (1914-1918) by a German chemist named Fritz Haber and his assistant in a laboratory. Later, in 1910, Carl Bosch took this idea and created a large-scale industrial machine for ammonia production.
In this article, we will learn What is Haber Process, the Diagram of Haber Process, equations, and thermodynamics involved in Haber’s Process.
Table of Content
- What is Haber’s Process?
- Raw Materials Used in Haber-Process
- Haber Process Diagram
- Haber Process Condition
- Thermodynamics of Haber Process
- Reaction Rate and Equilibrium of Haber’s Process