Toluene Reaction Lab Report

In week one of unit four, a bromination reaction is performed on trans-diphenylethylene. However, in week two, a dehalogenation reaction is performed on the product generated from week one. Both reactions featured the reflux set-up, which allowed the reactions to occur at higher temperatures and aided in the prevention of the evaporation of the solvent and the loss of product. Furthermore, the reactions were conducted in conjunction with the methods of green chemistry, which is a design of synthesis processes that minimizes the production of malignant compounds. The products from both weeks were further analyzed by several analysis tools utilized throughout the semester.

(b) Calculate the initial rate of absorption ofC12H26Sfrom a 1 mM solution at 20 °C ifits initial sticking coefficient is 1×10–6.6.A gas phase reaction between atomA and a diatomic molecule BC has a positive activationenergy to reach a collinear transition state. Describe how the reaction to form AB occurs.Suggest a plausible explanation for why the product AC is not formed.7.Calculate thecollision rateof waterwith a surface ifthe surfaceis exposed to (a) water vaporwith a pressure of 1 atm and (b) liquid water?The system is held at 350 K.8.The forward and reverse rate constants have been measured for the gas-phase reactionH2(g) +I2(g)2HI(g).The reaction is bimolecular in both directions with Arrhenius parametersA=4.45×105dm3mol–1s–1,Ea=170.3kJ mol–1(forward reaction)A'=5.79×101dm3mol–1s–1,Ea' =117.6kJ mol–1(reverse reaction)Computek,k' (rate constant for the reverse reaction),K,ΔrG°,ΔrH°, andΔrS° at

Diels-Alder Reaction Objective: The objective of this experiment is to demonstrate a typical Diels-Alder reaction by reacting anthracene (diene) with maleic anhydride (dienophile) to produce 9,10-dihydroanthracene-9,10-α,β-succinc acid anhydride, the product. Scheme 1. Cycloaddition through the Diels-Alder Reaction1 Experimental: Anthracene (1.00 g, 5.61 x 10-3 mol), maleic anhydride, (0.75 g, 7.65 x 10-3 mol), and xylene (5.0 mL) were combined in a 10 mL long-necked, round-bottomed flask. A stir bar was added and an empty distillation column was attached to the flask to function as an air condenser. The mixture was refluxed for 40 minutes over a sand bath, ensuring the temperature was monitored to prevent the reflux ring from surpassing the

When the xylene was added the mixture turned a light yellow. A condenser was attached to the round-bottom flask and mixture. The reaction refluxed and stirred for forty minutes on a sand bath. After forty minutes, the reaction cooled to room temperature. Then, the reaction was placed in an ice bath for ten minutes to allow crystallization. Next, the crystals were isolated using a vacuum filtration with Hirsch funnel. Also, the crystals were washed with ice-cold xylene (2 x 5

Review 2: Text In chemical kinetics, the reaction rate law is calculated experimentally to find how change in concentration affects change in rate, and to find a proportionality constant k, known as the rate constant. Since the instantaneous initial rates at various concentrations of A and B are provided, we must find the orders m and n of each reagent to determine the rate law, Rate=k[A]m[B]n. When A is doubled and B is held constant, the instantaneous initial rate approximately quadruples.

By comparing the relative reactivity rates between the different hydrogens to bromine, a hypothesized ranking of reactivity was made of the provided hydrocarbons: toluene, ethyl benzene, tert-butylbenzene, cyclohexane, and methylcyclohexane. This hypothesis was then tested during the actual lab period by preparing two sets of reactions for each hydrocarbon: one in light and one in dark. Observations were noted throughout a thirty minute period in order to determine the experimental order of reactivity. Free-radical chain reactions are one of the few mechanisms that allow for functional

Following its protection with a THP group, a second selective transmetalation occurs using iPrMgCl in toluene along with the addition of DMF. This results in an anion that corresponds with C-2 aldehyde (17). This aldehyde is condensed with N-tert-butyl azaindolene (18) in order to produce its Z-isomer (19). The Z-isomer (19), a highly crystalline alkene, is reduced with NaBH4 followed by THP deprotection, producing

For the Bromination of Toluene lab the ratio of the ortho, meta and para ratio in the bromotoluene product mixture was determined using quantitative IR spectroscopy. For the toluene to be mixed with bromine it must undergo Electrophilic Aromatic Substitution and it needs to be in the presence of a Lewis acid catalyst. Additionally, a metal staple must be used to generate a ferric bromide catalyst. The three products of brominating toluene are ortho-bromotoluene, meta-bromotoluene, and para-bromotoluene. There are five reactive sites on the aromatic ring where the hydrogen atom is replaced by a bromine, the ratio for this is 2:2:1 ortho, meta and para.

Chemical kinetics involving reaction rates and mechanisms is an essential part of our daily life in the modern world. It helps us understand whether particular reactions are favorable and how to save time or prolong time during each reaction. Experiment demonstrated the how concentration, temperature and presence of a catalyst can change the rate of a reaction. 5 runs of dilution and reaction were made to show the effect of concentration on chemical reactions. A certain run from the previous task was twice duplicated to for a “hot and cold” test for reaction rate. The prior run was again duplicated for a test with

Finally, the conversion is determined to be only 15.2 mol% with a low increment of 4.0 mol% (comparable to the increment of the blank test), attributable to the autoxidation of cis -cyclooctene by air. This result testi fi es the heterogeneity of the supported catalyst CoO x /Y. 3.5. Epoxidation of various cyclic alkenes Table 4 summarizes the catalytic performance of 2.4% CoO x /Y for the epoxidation of various cyclic ole fi ns with air. Comparatively, the reactivity of four ole fi ns decreases in a sequence of α -pinene (92.1 mol% conversion)

This experiment was sought out in order to further inorganic labs taught on Taylor University’s campus. The purpose of these experiments were to validate the ruthenium based catalyst RuH2(CO)(PPh3)3 and to find reactions that work well in Taylor’s lab setting using the synthesized catalyst. By reviewing several past experimentation, reactions were chosen based on several criteria: cost, time, technique and products produced. Through literature, we are able to either validate or discredit products based on data from Infrared Spectroscopy and Nuclear Magnetic Resonance. Removing the catalyst from the product, however, proved to be more difficult that anticipated. Through literature, it was found that the catalyst RuH2(CO)(PPh3)3 works well catalyzing

Also it is comprehended by review of academic literatures such as articles and dissertations that GTL is more attractive than any other XTL technologies. Although pipeline is a routine method for transmission of natural gas in countries with huge amount of this wealth [10] but GTL also have its own value in monetizing natural gas source to easily vendible liquid hydrocarbons. So many of researches devoted to different fields of GTL process merely, beside those investigations on the common part of all XTL technologies such as FTS and syngas production. Amongst these fields, catalyst is the most attractive issue in different fields such as promoters and formulation [11, 12], support [13], preparation …, and both cobalt and iron catalysts are matter of investigation as well as other new catalysts.

A way to approach the elimination of carbon monoxide from car exhaust is through the use of organometallic catalysts. Through the use of a catalyst, a reaction can occur at a faster rate and at lower activation energy. Said catalysts serve are of great commercial interest because they essentially convert simple mole-cules into more complex ones.6 Unlike homogeneous catalysts, heterogeneous catalysts are not in the same phase as how the reac-tion is occurring. Because of this, the catalysts are considered to be cheaper and easier to obtain. It is also considered more envi-ronmentally friendly to use.6-7

The catalyst used in this study is a Ni-Mo supported on alumina that is a bi-function catalyst and commonly used for HDT and HDC of heavy residue such as atmospheric residue. The specifications of catalyst are listed in Table (2).

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