EXPERIMENTAL RATIONALE Hydrocarbons are organic molecules consisting of hydrogen and carbon only1 and can be classified as saturated or unsaturated. A saturated hydrocarbon has the maximum number of hydrogens that can be present, given the number of carbons in the compound, for example, acyclic alkanes. A hydrocarbon is unsaturated if a hydrogen can be added1. This is a result of a hydrogen in the molecule being replaced, for example, with a double or triple bond or ring structure. Three examples of saturated or unsaturated hydrocarbons, used in the experiment are hexane, cyclohexane and cyclohexene, depicted in Figure 1. Figure 1: Table of comparison for each hydrocarbon Hydrocarbon Hexane Cyclohexane Cyclohexene Chemical formula …show more content…
Hucknall, David 2012, Chemistry of Hydrocarbon Combustion, Chapman and Hall, London 2. University of California, 2014, Index of Hydrogen Deficiency, viewed 13 August 2017, https://chem.libretexts.org/Core/Organic_Chemistry/Fundamentals/Index_of_Hydrogen_Deficiency_(IHD) 3. Brown, William 2017, Organic Chemistry, Cengage Learning, Dallas 4. Chapman, Brian 2003, Organic Chemistry, Energetics, Kinetics and Equilibrium, Thomas Nelson, Cheltenham 5. Solomons, Graham 2004, Organic Chemistry, J. Wiley & Sons, Tampa 6. Science Lab.com, 2005, Hexanes MSDS, viewed 17 August 2017, http://www.sciencelab.com/msds.php?msdsId=9927187 7. Science Lab.com, 2005, Cyclohexanes MSDS, viewed 17 August 2017, http://www.sciencelab.com/msds.php?msdsId=9927145 8. Science Lab.com, 2005, Cyclohexenes MSDS, viewed 17 August 2017, http://www.sciencelab.com/msds.php?msdsId=9923626 9. ‘Combustion of Hydrocarbons’ 2017, Student RiskAssess, viewed 17 August 2017,
The lab started off by measuring critical materials for the lab: the mass of an an empty 100 mL beaker, mass of beaker and copper chloride together(52.30 g), and the mass of three iron nails(2.73 g). The goal of this experiment is to determine the number of moles of copper and iron that would be produced in the reaction of iron and copper(II) chloride, the ratio of moles of iron to moles of copper, and the percent yield of copper produced. 2.00 grams of copper(II) chloride was added in the beaker to mix with 15 mL of distilled water. Then, three dry nails are placed in the copper(II) chloride solution for approximately 25 minutes. The three nails have to be scraped clean by sandpaper to make the surface of the nail shiny; if the nails are not clean, then some unknown substances might accidentally mix into the reaction and cause variations of the result.
Introduction The purpose of this lab was to compare simple distillations of two sets of liquids by graphing the boiling points. One set of simple distillation of two liquids were supposed to have a boiling point difference of bout 30C while the other set of simple distillations had a melting point difference of about 57C. Furthermore, by conducting this experiment, students would develop a better understand of distillation and gas chromatography. Furthermore, I hypothesized that cyclohexane and p-xylene distill better than cyclohexane and toluene since cyclohexane and p-xylene have a larger boiling point difference than cyclohexane and toluene. The boiling point of cyclohexane is 80.74C while the boiling point for p-xylene is 138.23C and the boiling point for toluene is 110.6, thus
The dehydration of 2-methylcyclohexanol takes place at the bottom of the Hickman still. As the Hickman still heats up within the sand bath, the products evaporate and travel higher up in the still where they condense into a liquid and fall within the collection ring, thus separating the product from the remaining water. Drierite (CaSO4) is also added as a drying agent to absorb any leftover water within the product. The purity of the product will then be analyzed with infrared spectroscopy, paying attention to OH peak if it is present. Chemical Reactions: Data and Observations: Material Volume Mol.
The chlorine atoms that are replaced by hydrogen atoms causes a higher presence and both are covalent bondings with strong intermolecular forces. The double bondings (Or triple bondings) in hydrocarbon tends to be stronger, but the chemical is flammable. Fluorocarbons are not flammable and are also polar covalent bondings, making them stable to ultraviolet radiation and prevents them from catalysing ozone depletion. Hydrochlorofluorocarbons (HCFCs), one of the alternatives that contains C-Cl bondings have most of its molecules dismantled in the lower atmosphere before reaching the stratospheric ozone layer. Another chemical, Hydrofluorocarbons (HFCs), having no chlorine atoms which does not bring harm to the ozone layer is considered the best alternative since they are not flammable, such as CF3CH2F,1,1,12 tetrafluoroethane.
It is possible that the discrepancy of the molecular weight of both acetone and the unknown volatile liquid was caused by the deviation of mass in each trial. During the trial of the experiment aluminum foil was used as a cap for the Erlenmeyer flask and by using a pin, a hole was made into the cap to insure that the gas vapors would escape during the heating process, later the Erlenmeyer flask was measured after the heating process when the gas was fully condensed; however, this procedure effected the results collected. With the usage of the aluminum foil it had resulted the presence of excess moisture build up from the water bath which then had increased the mass of the gas that had been condensed due to it being measure with both the foil and elastic band. Since, the Erlenmeyer flask was left behind with the water moisture contained in the foil; therefore, it had affected the final mass of the condensed vapor inside the flask. Although the procedure was effective and adequate results were obtained, there are some improvements that can be made towards the experiment to make it exceptional.
Conclusion: The five reactions are all oxidation of ethyne gas, which is an alkyne. The first four reaction is oxidizing the alkyne through combustion and the final reaction is through the use of KMnO4. The conclusions for the two sets of reactions, combustion reaction and catalyst driven reaction, is covered individually. Oxidation of Ethyne through Combustion (Tests #1 to #4, inclusive)
Acetic acid (CH3COOH) and formaldehyde (HCHO) can be obtained by processing methanol and is also used for petrol bending (petroleum derived liquid). A large proportion of methanol is used to make motor spirit, vinyl acetate, acetic anhydride these chemicals is used for the manufacture of adhesives, coating, photographic film, synthetic fiber, synthetic rubber and thermoplastic and mainly the methyl-tertiary butyl ether (MTBE) which reduces “knock” and also the proportion of CO and hydrocarbon in the exhaust. we can produce various aromatic hydrocarbons and alkanes suitable for petrol (hydro carbon with five to eight carbon atoms ) by throwing the stream of vapour over alumina at temp. around 600 kelvin. An equilibrium mixture of methanol, dimethyl ether and water is produced which has 25 percent methanol.
The crude oil is heated in a tall cylinder called fractionator for at least 350 degC. The process is based on the principle that different substances boil at different temperature. The cyclohexane content of naphtha fraction of crude oil can vary from 0.5 to 5.0 volume %. N-hexane, isohexanes, methyl cyclopentane, benzene and dimethyl pentanes have normal boiling points very close to cyclohexane.1 Advantages: 1. Uses a simple method of cyclohexane recovery. Disadvantages: 1.
Rediet Legese iLab Week # 6 CRUDE OIL DISTILLATION Introduction: The aim of this week lab experiment is to experiment distill crude oil and to check how temperature determine the chemical properties of crude oil plus how the boiling point can also show physical properties. They are two major finding in this experiment. he first finding was the point at which the raw petroleum is heated to the point of boiling, at 275 0C, the gas and kerosene oil are refined, however the oil (lubricant ) stays as an unrefined feature oil.
All day, everyday we come in contact with hazardous chemicals. These contaminants can be found in anything from plastic bottles to computers, from cosmetics to teflon pans, and from food we eat to the water we drink; the source of exposure is infinite. Chasing molecules by Elizabeth Grossman explores how these exposure happen and what occurs at the molecular level when we come in contact with these offenders. Elizabeth Grossman has researched many of these synthetic chemicals, which in our society are up to ninety percent petroleum based and she points out how our world needs to get away from such toxic chemical.
The peak area of the second fraction were 58.77% at ——— and 39.86% at ———-. The third fraction of hexane-heptane was collected, but the sample was not taken for distillation due to the teacher assistant’s specific instructions. The fourth fraction of the hexane-heptane mixture temperature ranges were not available. The peak of the fourth fraction appeared to be 24.29% at ——- and 75.71% at ——-. All three fractions of the hexane-octane mixture that were taken during the experiment were evaluated by a gas chromatogram.
It is commonly known throughout human history that the energy used is burned from coal which creates biomass. During the Industrial Revolution, coal was an essential need to everyone, hence the discovery of oil as a substitute. Yet, the mass formation from the unearthing of oil causes more damage than benefits for the planet. Humanity had never seen a more compatible source in which came a higher demand for oil. As the public has urged to generate more oil, scientists theorized that fossil fuels will eventually run out, making way for a renewable energy route in the future (Mason).
Introduction Strong acids and strong acids both dissociate completely in water forming ions. However, strong acids donate a proton to form H3O+ along with a conjugate base and strong bases accept a proton to form OH- along with a conjugate acid. The chemical behavior of acids and bases are opposite. When they are together, their ions cancel out and form a neutral solution. In this experiment, HCl and NaOH will react to form NaOH and H2O with these two steps: The overall reaction is: Both Na+ and Cl- ions combine to form NaCl.
Abstract The unknown concentration of benzoic acid used when titrated with standardized 0.1031M NaOH and the solubility was calculated at two different temperatures (20◦C and 30◦C). With the aid of the Van’t Hoff equation, the enthalpy of solution of benzoic acid at those temperatures was determined as 10.82 KJ. This compares well with the value of 10.27KJ found in the literature.
From the start of the industrial revolution to modern times, fossil fuels have been the go-to source of energy. Vehicles, homes, and entire cities rely on the use of fossil fuels to power the various technologies. However, this type of energy that many people depend on (oil, coal, and natural gas) are limited resources that will inevitably run out. But from the use of renewable resources, the energy produced by these technologies can replace part of the energy that comes from fossil fuels. In the past, the burning of fossil fuels was a unique innovation with little concern as to what it may face in the future.