Reaction Rate and Equilibrium of Haber’s Process
The Haber-Process is necessary for synthesizing ammonia through the reaction of nitrogen and hydrogen. This reaction is reversible reaction and that the forward reaction is exothermic involving the release of energy:
N2 (g) + 3H2 (g) → 2NH3 (g)
Nitrogen is obtained by separating it from the atmosphere through liquefaction, while hydrogen is obtained from the reaction of methane and steam:
CH4 (g) + H2O → H2 (g) + CO(g)
As per Le Chatelier’s principle, ammonia production is occurred at high pressure and low temperature. Typically, the Haber process operates within the range of 200 to 400 atmospheres at a temperature of 500°C. In the industrial production of ammonia, the continuous removal of NH3 ensures the continuity of this reaction.
This reversible reaction is influenced by changes in temperature, pressure, and the catalyst applied. It impacts the composition of the equilibrium mixture, the reaction rate, and the overall economic feasibility of the process.
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
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