Haber-Bosch control room
About this app
Run temperature and pressure right at the reactor and switch catalyst and removal: particle groups change atom by atom between N₂ + 3 H₂ and 2 NH₃, and three displays separate equilibrium fraction, rate and yield per hour. Why the best position is not the best result, with five experiments, a prediction of the optimum and exam questions.
With explain mode: an AI tutor walks you through the app, points out what matters in the scene and answers your questions.
What it is about
The ammonia synthesis N₂ + 3 H₂ ⇌ 2 NH₃ is exothermic and lowers the number of gas particles. By Le Chatelier, low temperature and high pressure improve the position of equilibrium. At low temperature, however, the reaction is slow, and the gas stays in the reactor for a limited time only. The best equilibrium position is therefore not automatically the best result. The goal is the highest yield per time, and that lies at a compromise.
What the app shows
A reactor in section shows particle groups that switch atom by atom between four molecules N₂ + 3 H₂ and two molecules NH₃. Columns stand for temperature and pressure, and a loop leads back through a separator. Three displays give the equilibrium fraction, the share reached and the yield per hour. The equilibrium values come from tables for a 3:1 mixture. The rate is a model assumption, and the optimum of 450 °C at 200 bar is tuned to it. The model does not count costs.
What you try out
You drag the knobs on the columns, switch the catalyst and removal and read from three charts what limits the yield. Five experiments lead through position, rate, catalyst, compromise and loop. In the prediction you fix your temperature for the optimum before the yield curve appears. Seven exam questions cover Le Chatelier, Kp, conversion and the role of the catalyst.
Frequently asked questions
- Why does the Haber-Bosch process not run at the lowest possible temperature?
- Low temperature improves the position, but the reaction becomes slow. In its time in the reactor the gas reaches only a small part of equilibrium. In the app’s model 300 °C at 200 bar gives 64 % NH₃ at equilibrium, but the gas reaches only 7 % of that. At 450 °C the figures are 27 % and 78 %, and the yield per hour is higher.
- Does the catalyst change the position of equilibrium?
- No. It lowers the activation energy for forward and reverse reaction alike. Equilibrium is reached sooner and the equilibrium constant K stays the same.
- Why is ammonia removed from the loop gas?
- Without NH₃ the reaction quotient Q lies below K, so the forward reaction prevails. If the ammonia stayed in the gas, Q would approach K and there would be no net product any more. The remaining gas circulates and reacts on the next pass.
- What can I do in the app myself?
- You run temperature and pressure, switch catalyst and removal and predict the optimum. An explain mode goes from cold to hot and shows where the yield is highest.
Subject: Chemistry
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