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Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
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leolena leolena
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11 years ago
The Haber process produces ammonia from nitrogen and hydrogen in an exothermic reaction. It is an equilibrium process, which means there is always a balance between the reactants and products. The challenge is to optimize conditions for the maximum production of ammonia.

Based on what you know of Le Chatelier's Principle, what conditions of temperature and pressure should be used to maximize the amount of ammonia produced? Explain your answer.
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#1
11 years ago
N2(g)  +  3H2(g)     Leftwards Arrow>  2NH3(g)
The reactant represents 4 volumes of gas, while the product represents only two volumes'
Adding more reactant encourages more product to form in order for the pressure to regain equilibrium
Since the reaction is exothermic it should be done at a low temperature in order to remove the heat, which is a product..
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