Essay on The Haber Bosh Process and the Importance of Making Ammonia

Abstract: This two part experiment is designed to determine the rate law of the following reaction, 2I-(aq) + H2O2(aq) + 2H+I2(aq) + 2H2O(L), and to then determine if a change in temperature has an effect on that rate of this reaction. It was found that the reaction rate=k[I-]^1[H2O2+]^1, and the experimental activation energy is 60.62 KJ/mol.

This experiment was conducted under conditions described by Williamson, 2003. To begin, approximately 150 mg of cyclohexanone was placed into a vial. In a separate 10 x 100 mL reaction tube, 1.0 mL of HNO3 was added by pipette, along with a pre-weighed boiling chip. The reaction tube containing the nitric acid was clamped into a sand bath under the fume hood and heated at a low setting. One drop of cyclohexanone was careful added to the nitric acid. The presence of a brown oxide indicated that the reaction had begun, at which point the reaction tube was removed from the sand bath.

Purpose: The purpose of this experiment is to observe a variety of chemical reactions and to identify patterns in the conversion of reactants into products.

Experiments 2-1 and 2-2 study the production of hydrogen gas by different chemical reactions. By using a hydrogen gas collection apparatus and the principles of chemistry, we were able to evaluate the data and reach our goal. Experiment 2-1 uses zinc, magnesium and aluminum and how much hydrogen gas they produce to predict the volume of hydrogen gas produced for different masses of each metal. In this experiment we see that each metal has an increasing amount of hydrogen gas as mass goes up, however each metal had different amount of hydrogen gas for the same mass. Zinc produced the least amount of hydrogen gas, then increasing with magnesium, and aluminum produced the highest amount. The

It is not “naturally occurring” and it is not composed of only ammonia, phosphorus and hydrogen sulfide” (Hunter-Burch, 2005, n.d.).

By increasing the temperature as increasing the temperature increases reaction rates because of the disproportionately large increase in the number of high energy collisions. This could have been done by warming the water instead of using room temperature.

Most importantly, they require phosphorus, nitrogen, and potassium for making phospholipids (which make up the cell membranes), amino acids, and metabolic functions.10 This is why most fertilizers contain some combination of these three elements. Sulfur also plays an important role in plants, as it helps form amino acids, proteins, and chlorophyll11. Because these elements are all important to plant growth and are common ingredients in fertilizers, they were used to create a liquid fertilizer in this lab. (Note that only Day 2 of the lab used

The reaction is carried out in saturated aqueous ammonium chloride solution. Thus no special drying of solvents, reagents, or glassware is required. The reaction mechanism for this experiment can be seen below (Fig. 2)

The Haber Process has many positive implications. It allows nitrogen to be pulled directly from the atmosphere,

The nitrogen cycle is extremely important. This is because of the importance of nitrogen itself. Nitrogen is a basic element of life. It also makes up 78 percent of the Earth's atmosphere. It forms an essential part of amino acids (which make up proteins) and DNA. Nitrogen is essential for all living cells.

The pipet was put into the top of the condenser and leaving no open spaces. The vacuum served to get rid of the nitrogen oxide gases that were formed during the oxidation reaction. The solution was heated for 30 minutes, beginning the time when the first sign of nitrogen oxide fumes were observed. After the 30 minutes, the solution was removed and cooled for a few minutes. The solution turned was a brownish-yellow color and all the crystal were dissolved, leaving a liquid. The solution was then transferred, using a Pasteur pipet, to 3 mL of water in a beaker. The reaction flask was rinsed to remove the remainder of the solution. The solution was stirred with a glass rod until room temperature of the solution was achieved. A yellow solid was to form, but instead the solution remained aqueous in the case of the specific experiment explained here. With additional scraping of the solution with a glass rod, no crystals formed at all. The next procedure, if the crystals had formed was to crush the solid with the glass rod and filter the solid until the crystals were dry. The mass would then be weighed and the crystals were to be recrystallized with 95% ethanol. The crystals were to be cooled in ice water to get full crystallization and then the crystals were to be filtered and air dried, then weighed.

Fritz Haber was the director of the Kaiser Wilhelm Institute for Physical Chemistry at Berlin-Dahlem (“The Use of Poison Gases in the First World War”). The earliest gases created by the Germans were acquired from Haber’s work, which was designed to synthesize ammonia from the nitrogen present in the air (“The Use of Poison Gases in the First World War”). Chlorine was the first war gas. This gas was installed in the German trenches during 1915. In the date of April 22, 1915 a German plane dropped a cylinder container that released a greenish fume, recognized as poisonous chlorine gas.

Eutrophication, a term that derives from two greek words, eu, meaning “good,” and trophic, meaning nutrition or nourishment, is the enrichment of water bodies with nutrients like nitrogen and phosphorous that stimulate plant growth. Nitrogen is often found in rocks, soils, organisms, and the atmosphere; phosphorous resides mostly in rocks/soils and organisms. Having nitrogen and phosphorus in the ecosystem isn 't necessarily a bad thing, in fact, it 's required. Nitrogen is needed for the production of proteins and amnio acids, while phosphorous is required for the synthesis of DNA and RNA, and is involved in energy transfers. (Danver & Burch, 2011) However, too much of a good thing, can be a bad thing.

The goal of this source is to inform others how ammonia fits into the chemistry as well as hydrogen peroxide.

The conditions for this type of reaction vary depending on what degree of alcohol you are trying to oxidize. In our case, we oxidized a secondary alcohol at room temperature. It was