La Chateliers Principle free essay sample

For this assignment you will research one of the equilibrium systems below, or one approved by your instructor, and prepare a presentation describing the system. The Haber Process (or Haber-Bosch Process) The Haber process is the process for converting nitrogen and hydrogen from natural gas into ammonia. Control Click to follow link. The Haber Process PPT. ppt Questions to Answer Questions that should be answered by the content of your research project: 1. Describe the process you researched, including its uses in various industrial or health fields. I chose to research The Haber Process. We will write a custom essay sample on La Chateliers Principle or any similar topic specifically for you Do Not WasteYour Time HIRE WRITER Only 13.90 / page It combines nitrogen from the air with hydrogen that comes from natural gas, into ammonia. The reaction is reversible and the production of ammonia is exothermic. 2. Who developed or discovered this process? When? What country was he or she from? (Provide this information if you can find it. ) Fritz Haber, a German Chemist was the person who developed The Haber Process. He had developed it in 1905. Fritz Haber is from Germany. 3. Provide a short paragraph providing some historical background. Why is, or was, this an important chemical process? The Haber Process was developed at the time leading up to WWI. By 1914, German chemical engineer, Carl Bosch had helped Haber in converting the method into an industrial process. This was a very important chemical process because it produces ammonia which is used to make fertilizers, explosives, dyes, household cleaners, and nylon. 4. Write a balanced chemical equation for this reaction, including the energy term. Is it an endothermic or exothermic reaction? N2(g) + 3H2(g) 2NH3(g). The production of ammonia is exothermic. Use Le Chatelier’s principle to explain the conditions that favor the forward reaction. The position of the equilibrium will shift in a direction that helps to reduce the effect of that change as long as a change is imposed on a system at equilibrium. 6. Under what temperature, pressure, and other conditions is this reaction typically carried out? How does this relate to part of your answer for Question 3? Nitrogen and hydrogen could be combined at elevated temperatures and pressures, in the presence of a catalyst (a process in which Haber first demonstrated, in 1905) 7. What safety, cost, or other considerations prevent most industrial applications from using the most ideal conditions for high yield of the product? Most industrial applications are prevented from using the most ideal conditions for high yield of the product, most likely due to a lack of knowledge in building the high pressure equipment that is needed to carry out the reaction. 8. What catalyst, if any, is used for this reaction? One catalyst could be a mixture of iron and iron oxide. Efficiency could be increased by adding aluminum.