N2( g)+3 H2( g) (Fe / Mo, 500^∘ C)/(V 200-900 atm) 2 NH3+22.4 kcal formation of NH3 by above re

step 1 In this problem, we have given a reaction in 2 gas reacts with 3 moles of H2 gas reversibly and

N2( g)+3 H2( g) (Fe / Mo, 500^∘ C)/(V 200-900 atm) 2...

$\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \frac{\mathrm{Fe} / \mathrm{Mo}, 500^{\circ} \mathrm{C}}{\mathrm{V} 200-900 \mathrm{~atm}} 2 \mathrm{NH}_3+22.4$ kcal formation of $\mathrm{NH}_3$ by above reaction shows (a) Cyanamide process (b) Serpeck's process (c) Haber process (d) None of these

$\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \frac{\mathrm{Fe} / \mathrm{Mo}, 500^{\circ} \mathrm{C}}{\mathrm{V} 200-900 \mathrm{~atm}} 2 \mathrm{NH}_3+22.4$
kcal
formation of $\mathrm{NH}_3$ by above reaction shows
(a) Cyanamide process
(b) Serpeck's process
(c) Haber process
(d) None of these

Key Concepts

Chemical Equilibrium

Chemical equilibrium principles are central to understanding industrial reactions, including the synthesis of ammonia. Equilibrium considerations dictate how temperature and pressure adjustments can be used to favor the production of ammonia, particularly in exothermic reactions where the release of heat must be managed to maintain optimal conversion rates.

Reaction Conditions

The reaction conditions in industrial processes, including high pressure and controlled temperature, are essential to shifting the chemical equilibrium in favor of product formation. For exothermic reactions like ammonia synthesis, these conditions help to optimize the balance between reaction rate and equilibrium yield, ensuring efficient production in an industrial setting.

Haber Process

The Haber process is a major industrial method for synthesizing ammonia by reacting nitrogen with hydrogen in the presence of a catalyst. This process is significant because it converts relatively inert atmospheric nitrogen into ammonia, which is a precursor for fertilizers and numerous chemicals, and it involves careful control of reaction conditions to maximize yield.

Industrial Catalysis

Industrial catalysis involves using substances such as iron, often alloyed with promoters like molybdenum, to accelerate chemical reactions without being consumed in the process. In ammonia synthesis, these catalysts play a crucial role in lowering the activation energy and improving the efficiency of the reaction under the high-pressure and moderate-temperature conditions required.

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