Oxidation Of Hydrocarbon Essay

In radical halogenations lab 1-chlorobutane and 5% sodium hypochlorite solution was mixed in a vial and put through tests to give a product that can then be analyzed using gas chromatography. This experiment was performed to show how a radical hydrogenation reaction works with alkanes. Four isomers were attained and then relative reactivity rate was calculated. 1,1-dichlorobutane had 2.5% per Hydrogen; 1,2-dichlorobutane had 10%; 1,3-dichlorobutane had 23%; and 1,4-dichlorobutane had 9.34% per Hydrogen.

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.

In this experiment, meso-stilbene dibromide was used to produce diphenylacetylene through two sequential dehydrohalogenations. The first part is a concerted E2 mechanism, where the reactant is deprotonated at the beta carbon from the halide ion that will be leaving. This creates a transition state where the leaving hydrogen and halide are anti-periplanar with each other, meaning that they are at a 180° angle in relation to one another. This reaction is caused by a base—in this case, potassium hydroxide—and produces a haloalkene, or vinyl halide. Potassium hydroxide was only added to reaction when needed, as

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.

The purpose of this study was to conduct a Diels-Alder reaction with the reactants, anthracene-9-methanol and N-methylmaleimide, in conjunction with the principles and metrics of green chemistry: increasing atom economy, utilizing safer solvents, and preventing pollution.1 Upon completion of the calculation, the atom economy and percent yield were found to be 100% and 4.88% respectively. Subsequently, melting point range analysis yielded a melting range of 218-220℃. These findings could be useful for individuals looking to maximize the percent yield for other Diels-Alder reaction while utilizing benign green reagents and solvents.

In this week’s lab experiment, the rate of decomposition of hydrogen peroxide forming oxygen gas will be observed and studied. Since the rate of a chemical reaction is dependent on two things; the concentrations of the reactants and the temperature at which the process is performed, the rate can be measured at which a reactant disappears or at which a product appears. When measuring the rate, the rate law will be applied. The objective of this lab is to demonstrate how the rate changes with varying initial concentrations of hydrogen peroxide by measuring the rate at which oxygen is evolved.

Dane, John, and Kent J. Voorhees. "Investigation of Nitro-Organic Compounds in Diesel Engine Exhaust." National Renewable Energy Laboratory (2010). Print.

The melting point of the final product, diphenylacetylene, was found to be 65-68 degrees Celsius which is right around the ideal 61 degrees Celsius melting point; this shows that purification during the lab worked and that the sample was almost 100% pure. Since only 0.01g of diphenylacetylene was collected and the theoretical yield was calculated to be 0.049g, this experiment had a 20.41% yield. A few sources of error that explain the low percentage could be the loss of crystals when transferred from the test tube to the suction apparatus or when they were transferred from the suction apparatus to the filter paper to be dried and then weighed. Crystals could have also been lost if more than 5 drops of methanol was added because excess methanol would dissolve the crystals. The experiment was successful when looking at the crystals collected from the addition step and the elimination step; however, to improve the percent yield and collected product the the test tubes could have been allowed to cool down in the ice bath past the 5 minutes to ensure all the crystals formed

5.Position gas collecting hose so it runs from reaction vessel through gas collecting box to opening of the graduated cylinder. The idea is that any gas coming through the tube will rise in the graduated cylinder and displace the water in it.

Most aviation jet fuels are derived from Kerosene. Kerosene molecules can have varying numbers of carbons. It can have as little as 12 or as many as 15. This means the chemical formula can be anywhere from C_12 H_26 to C_15 H_32. (FOUR). From these basic chemical structures stem those that form JP-8, Jet-A, and other jet fuels. Jet-A is the lowest grade of fuel made from kerosene molecules. Typically available only in the United States to civilian aircraft, Jet-A varies from 8 to 16 carbon atoms per molecule. Jet-A1 fuel is nearly identical to Jet-A, except that it is manufactured to a higher standard as Jet-A, and is therefore available worldwide. Jet-A1 also contains between 8 and 16 carbon atoms per molecule. JP-8, also commonly known as NATO F-34 by other nations, is Jet-A1 with a package of additives specifically designed for military aircraft. These additives allow static dissipation, corrosion reduction, lubrication, anti-icing, and sometimes anti-oxidation and metal deactivation (FIVE).

It was desired to compare a theoretical value of enthalpy of combustion to a literature value. To do this, the theoretical value was calculated using a literature value for the heat of sublimation of naphthalene, the heat of vaporization of water and average bond energies, given in Table 1 of the lab packet.1 Equations (1) and (5) were used to calculate the theoretical enthalpy of combustion of gaseous naphthalene, where n was the number of moles, m was the number of bonds, and ΔH was the average bond energy:

A & C: MEASURING THE OPTICAL ROTATION OF CAMPHOR SAMPLES AND CAMPHOR OBTAINED FROM OXIDATION OF ISOBORNEOL

The purpose of this experiment was to test and observe the physical and chemical properties of gases, and to use these properties to identify these gases when they are encountered.

In this natural gas liquid (LNG) separation study conducted by Long and Lee (2011), the base separation system includes a sequence of depropaniser, debutanizer and deisobutanizer which separated a system the includes ethane, propane, n-butane, i-butane and heavies (C5+) (Long and Lee 2011). The demethanizer and deethanizer was

When oxyhydrogen kit is connected, hydrocarbons might have undergoing complete combustion or tend to follow complete combustion by the aid oxygen which is a part of oxyhydrogen. Also the chance for increased combustion duration also exists.