07.05 Le Chatelier's Principle Research Project
07.05 Le Chatelier 's Principle Research Project
Fritz Haber was born in December of 1868, in Prussia to a German chemical merchant. He went into the field of organic chemistry at the University of Jena. He was appointed as director of the Kaiser Wilhelm Institute for Physical Chemistry in Berlin in 1911. He was in charge of forming a center for cross-disciplinary research and gave his country the knowledge of ammonia and other significant fertilizers. He left Germany in 1933 after their loss in WW1, and passed away in Switzerland in 1935. The Haber Process combines nitrogen from the air with hydrogen from natural gasses like methane into ammonia. This process is a reaction that 's reversible and the production of ammonia is exothermic. …show more content…
To produce ammonia, the temperature must stay at a level that is low enough to the point where the reaction will continue in a forward direction. The temperature used is 450 to 500 degrees celsius. The pressure is used at 200 atmospheres with iron being the catalyst. The proportions of nitrogen and hydrogen in a 1/3 ratio is a correct stoichimoetric ratio for the reaction because most reactions use excess reactants to increase the yield, according to Le Chatelier 's principle. The temperature is 400-500 degrees celsius. The reaction is 15% efficient at this temperature, but has potential to occur at a rate that makes it viable. Pressure plays an important role in the equilibrium position of the reaction because there are 4 molecules on the left of the equation, but only 2 on the right. The Harber Process has a history with fertilizers and explosives. Ammonia from certain plants were more expensive to use in fertilizers than the ones that came from other products of other reactions. During WW2, an increase of demand led to cheaper and more efficient methods. Ammonia in the US is the second most important chemical, as nitrogen makes number
Fritz Haber was born in December of 1868, in Prussia to a German chemical merchant. He went into the field of organic chemistry at the University of Jena. He was appointed as director of the Kaiser Wilhelm Institute for Physical Chemistry in Berlin in 1911. He was in charge of forming a center for cross-disciplinary research and gave his country the knowledge of ammonia and other significant fertilizers. He left Germany in 1933 after their loss in WW1, and passed away in Switzerland in 1935. The Haber Process combines nitrogen from the air with hydrogen from natural gasses like methane into ammonia. This process is a reaction that 's reversible and the production of ammonia is exothermic. …show more content…
To produce ammonia, the temperature must stay at a level that is low enough to the point where the reaction will continue in a forward direction. The temperature used is 450 to 500 degrees celsius. The pressure is used at 200 atmospheres with iron being the catalyst. The proportions of nitrogen and hydrogen in a 1/3 ratio is a correct stoichimoetric ratio for the reaction because most reactions use excess reactants to increase the yield, according to Le Chatelier 's principle. The temperature is 400-500 degrees celsius. The reaction is 15% efficient at this temperature, but has potential to occur at a rate that makes it viable. Pressure plays an important role in the equilibrium position of the reaction because there are 4 molecules on the left of the equation, but only 2 on the right. The Harber Process has a history with fertilizers and explosives. Ammonia from certain plants were more expensive to use in fertilizers than the ones that came from other products of other reactions. During WW2, an increase of demand led to cheaper and more efficient methods. Ammonia in the US is the second most important chemical, as nitrogen makes number