Arrhenius vs. Le Chatelier battle

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SUMMARY

The discussion centers on the conflicting principles of Arrhenius and Le Chatelier in the context of ammonia reactor design. Arrhenius emphasizes the importance of high temperatures for reaction rates, while Le Chatelier advocates for lower temperatures to favor product equilibrium. This inherent conflict necessitates finding an optimal temperature that balances reaction speed and product yield, ultimately impacting ammonia conversion efficiency.

PREREQUISITES
  • Understanding of Arrhenius equation and its implications on reaction rates.
  • Familiarity with Le Chatelier's principle and its application in chemical equilibria.
  • Knowledge of ammonia synthesis processes and reactor design principles.
  • Basic thermodynamics related to chemical reactions.
NEXT STEPS
  • Research optimal temperature ranges for ammonia synthesis in industrial reactors.
  • Explore kinetic studies related to Arrhenius and Le Chatelier principles.
  • Investigate advanced reactor designs that integrate both principles for improved efficiency.
  • Learn about catalyst selection and its impact on reaction rates and equilibrium shifts.
USEFUL FOR

Chemical engineers, process designers, and students studying chemical kinetics and equilibrium, particularly those involved in ammonia production and reactor optimization.

member 392791
Hello,

In my class we were talking about the design of an ammonia reactor, and there is a battle between arrhenius and le chatelier for getting the highest conversions. Apparently the two are at odds with each other as far as getting the highest conversion of ammonia.

I am confused how the two, that separately both can be used to increase the products, have incompatibilities to fully utilize both of them to get the best conversion possible.

Sorry if this sounds vague, but I figured the thought of a fight between Le chatelier and arrhenius would spark interest
 
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Nothing new. You want a high temperature fro the reaction to be fast, you want low temperature for the equilibrium to lie on the right, so you need to find some kind of optimum to be able to produce as much as possible of the final product in the time unit.

Please disperse, there is nothing to see. Same old thing, repeated in all chemistry all around.
 

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