Hydrate Essays

2.8 Gas Hydrates Challenge Gas hydrates is a major flow assurance challenge in long distance multiphase flow line. For better understanding of this phenomenon, gas hydrate would be looked at under the following headings: 1. A brief history of Natural gas, 2. The components of natural gas, 3. A brief history of natural gas hydrates, 4. The Basic structure of gas hydrates, and the conditions that are necessary for hydrates formation, 5. Hydrate formation and growth in pipeline. 2.8.2 A Brief History

some compounds attract and form bonds with water molecules, forming hydrates. A hydrate is a salt that has water molecules trapped within its crystals. Every hydrate has a certain number of water molecules weakly bonded to the salt as follows: salt • number of water molecules Anhydrous salts are salts that can form hydrates but which have had all the water driven off, usually by heat. By heating the Copper (II) sulphate hydrate until its color changes from blue to white, the compound can be decomposed

In the lab, “Properties of Hydrates,” the purpose was to compare the properties of several well observable hydrates and to determine if dehydration is a reversible or irreversible change. The lab consisted of attaining a pea-size sample of each compound, burning it over a bunsen burner, and comparing the starting mass and the mass lost after the combustion. These results are important to be able to identify a variety of different chemicals that contain water molecules as part of their crystalline

Hydrates are names given to compounds that contain water molecules with the formula of H2O, usually containing a fixed value of water mass percentage (Kauffman, 1998). The experiment performed consisted of three main parts. First, different hydrated salts were heated in test tubes with a Bunsen burner in order to determine observational changes for before, during, and after dehydration. After dehydrating the salts, water was added back into the test tubes to determine if rehydration was possible

As for my part in this company, I feel the best role that I would excel at for the Educate to Hydrate organization would be the part as an Advocacy Director. For my Myers-Brigg results, I am an ESFJ personality type. I am a detail-oriented person and I plan ahead of time of my goals, schedule conflicts, and time management in order to avoid procrastination. These skills could be incorporated into identifying Educate to Hydrate’s advocacy goals and strategies. I also feel that in building relationships

Gas hydrates The chemical structure of a gas hydrate includes only water and a given gas molecule (e.g. methane or carbon dioxide). When hydrates form, the chemical structure excludes all salts and other impurities. When the hydrate is dissociated, only gas and pure water remain. Rapid spray evaporation Rapid Spray Desalination (RSD) is a new technology that makes efficient use of waste heat generated from gas-fired electrical generating plants, wastewater treatment plants, landfills, and other

Introduction Gas hydrates also known as clathrates have been known for about 200 years. For over 60 years they have been studied by oil and gas industries. According to (Cranganu and Nitzov), It wasn’t until about 18 years ago many publication companies covered articles about the potential energy sources they could be as well as Characterization, Carbon Sequestration, geophysics, and Global climate changes. Over the recent years it’s been a high demand for finding new sources of energy that were

In this project, titanium(IV) ethoxide, Ti(CC2H5)4, Cobalt(II) nitrate, Co(NO3)2.6H2O, Iron(III) nitrate-9-hydrates, Fe(NO3)3.9H2O, and strontium nitrate, Sr(NO3)2 are needed to prepare both non-substituted strontium ferrite and substituted strontium ferrite. In this case, non-substituted strontium ferrite acts as a control in this project to compare with the characteristics of cobalt-titanium substituted strontium ferrite. The main objective of this project is to compare the effect of substitution

experiment is to find out what is the identity of the unknown hydrate? To answer this question first, we should know what a hydrate, and how to identify a hydrate using the law of constant proportions. A hydrate is a pure substance because it contains water molecules embedded in its crystal structure that does not vary. By heating the unknown hydrate, we can calculate the mass of the hydrated, and the percentage of water in the hydrate. To begin this, experiment our group start to weigh three difference

Kendrell Goodwin Formula of a hydrate Objective/hypothesis The objective of this lab is to calculate the number of moles of the anhydrous salt and the moles of water driven off. The purpose of this lab is to determine the formula of the hydrated salt. The outcome expected in this lab is that the Procedure Get a porcelain crucible and cleanse with soap then rinse with tap water. Follow up after rinsing with tap water, with rinsing with distilled water. Place the crucible on the iron ring of the

Hydrates/ solvates The stoichiometric type of adducts where the solvent molecules are incorporated in the crystal lattice of the solid are called as the solvates. When the solvent in association with the drug is water, the solute is known as a hydrate. Generally the anhydrous form of drug has greater solubility than the hydrates. This is because the hydrates are already in interaction with water and therefore have less energy for

pros for the methane hydrate divide into 3 part. First,Methane hydrates have great amount in seabed. “Estimates suggest that there is about the same amount of carbon in methane hydrates as there is in every other organic carbon store on the planet,” Methane Hydrates have a huge reserve on the edge of continental shelves where the seabed drops sharply away into the deep ocean floor.It can be the alternative energy to lower the consumer of the coal and oil. Second,methane hydrates is a high efficiency

Finding the Formula of a Hydrate – Lab Report (DCP, CE) Introduction and Overview: A hydrate is a chemical that has water molecules loosely bonded to it. The water molecules are not actually part of the formula, so the formula is written slightly differently. An example would be CaSO4 . 3H2O. This chemical would be called calcium sulfate trihydrate. When finding the mass of this chemical, you find the mass of the calcium sulfate and then add 3 times the mass of water to it. (40.08 + 32.066

Title : Determination of chemical formula of hydrate Aim To determine the chemical formula of hydrated Copper (II) sulphate, CuSO4 Research Background “When the chemical is heated the hydrate will convert to an anhydrous ionic compound (this means the water will leave it). The moles of H2O will be determined by assuming the amount of mass lost by heating is the mass of the evaporated H2O. The moles of the CuSO4 (the white substance after heating) can be calculated from the mass of the white crystals

2.12 Hydrate Formation and Growth in Pipeline. As discussed above, Hydrate formation begins when fluid temperature drops below a certain level and starts to nucleate close to the hydrocarbon phase on a water droplet in gas, oil or condensate phases. Hydrates grow along the surface of a droplet, until it is completely covered with a thin hydrate layer. Then, water will penetrates from the interior of the water droplet to the surface of the hydrophilic hydrate surface next to the hydrocarbon phase

Percentage Composition of Hydrates The Introduction: Hydrates are ionic compounds and are often a type of salt with a definite amount of water as part of their structure. Hydrates are decomposed into anhydrous salt, a no-water compound, and water vapor when heat is applied; water vapor is released from the hydrated compound, which leaves with an anhydrous salt that weighs less than the hydrate. But how do we find the percent of the water that was lost after applying heat to the hydrates and how accurate

The thought of having to undergo surgery without any type of anesthetic is quite unfathomable. Anesthesia is something that people take for granted and its importance is often overlooked. Until the eighteenth century, anesthetics were typically concocted by herbalists from the plants and flowers available to them. Surgeons would use an opioid concocted from poppy flowers on a sponge through means of inhalation to subdue their patients. As the practice of medicine has progressed, the methods used

was used. First, the vials were cleaned of impurities using the lab oven and were not touched after this point. The 2 vials were then weighed and vial 1 weighed 14.7681 grams and the second vial weighed 14.7451 grams. Next 1.1075 grams of the hydrate was added into vial one and 1.1015 grams was placed into vial 2. The vials were then placed back into the oven with a starting weight of 15.8756 for the first vial and 15.8466 grams for vial 2. Once they were taken out of the oven and cooled they

collection in Part I (table 1.2) it appears that there were several reactions that were reversible and some that weren’t. Copper Sulfate showed the most prevalent reversible reaction by returning to its natural blue color. However, the texture of the hydrate had transformed from small blue crystals to a smaller grain size. Cobalt Sulfate had similar characteristics beginning with large purple crystals which after being re-hydrated gained its original color back but also conceived several blue specs. Ferrous

calculated that we had 0.013 moles of water. After that we used the same formula to calculate the number of moles of our hydrate which was 0.005 moles. We then divided the number of both moles with the smallest number of moles of what we found. Therefore, we did 0.005/0.005 and 0.013/0.005 and we got the answer one and three respectively. So, the number of molecules in our hydrate was