In this lab, the objective was to examine the effect of an SN2 reaction using a phase transfer catalyst in dichloromethane. We isolated the product of the phase transfer reaction by using liquid chromatography and then prepared TLC plates to see which of the five vials collected contained the isolated product and an IR spectrum was then obtained. The reaction in this lab was an example of an SN2 reaction. SN2 is a nucleophilic substitution reaction where one bond is broken and one bond is formed in one step. For example, a lone pair from the oxygen in naphtholate anion attacks the carbon that is bonded to bromine from an allyl bromide molecule. This creates a partial C-O bond and a partial broken C-Br bond, then the C-O bond fully bonds …show more content…
The first visible peak was an sp3 C-H stretch at 3058.54 cm-1. The next peak was a C=C stretch at 1600.05 cm-1 and at 1628.97 cm-1. There was also a peak of an sp3 C-H bend at a range going from 1363.15 cm-1 to 1469.71 cm -1. The next peak was a C-O stretch at 1215. 40 cm-1. At the fingerprint region, there was an intense peak at 734. 51 cm-1, which could be the C-CL stretch found in dichloromethane, which means the product might not have been pure. This lab was successful to an extent because we were able to obtain the product, 2-naphthyl ether, but it was not pure since the IR spectrum showed traces of dichloromethane. Also the percent yield of the product was over 100%. Some sources of error in this experiment were that since the product in vial 3 had solidified, we had added a drop of dichloromethane to the vial, resulting in the C-Cl peak of the IR spectrum. Another error was that since the percent yield was over 100, there was an error in obtaining the mass of the vials because the same balance was not used. Also, the addition of the dichloromethane could have added to the mass and when calculating the percent yield, the mass of the dichloromethane was
Introduction An unimolecular substitution reaction, SN1 reaction, has a two step mechanism that results in a halide group being displaced by a nucleophile1. In an SN1 reaction, the first step involves the leaving of a halide group to form a carbocation intermediate. This is the rate determining step, and it is also the slowest step. In the second step a nucleophile attacks a face of the the carbocation. Figure 1 displays this mechanism.
Experiment VIII was performed to analyze SN2 and SN1 using tertiary and primary substrates and use gas chromatography (GC) to examine the SN1 reaction. The product of the SN2 reaction was classified as n-butyl iodide by using infrared spectroscopy and gas chromatography mass spectroscopy and the product of the SN1 reaction was identified as of t-butyl chloride by using infrared spectroscopy and gas chromatography. For the SN2 reaction, 7.62 grams of n-butyl bromide, 20.0 grams of sodium iodide, and 79.1 grams of acetone were used to produce 3.12 grams of n-butyl iodide. The limited reagent was identified as n-butyl bromide and the theoretical yield of n-butyl iodide was calculated as 10.3 grams. The percent yield of this reaction was calculated
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.
This shows that some impurities are present in the final product. Similarly, the experimental percent yield of 120.2% shows that some issues arose during the procedure. It is impossible to produce a pure product with over 100% yield; therefore, other impurities were present in the product that added weight to the finial mass. This extra weight pushed the yield well over 100%. This source of error could be due to a lack of drying the final product.
Abstract In this experiment, the reaction kinetics of the hydrolysis of t-butyl chloride, (CH3)3CCl, was studied. The experiment was to determine the rate constant of the reaction, as well as the effects of solvent composition on the rate of reaction. A 50/50 V/V isopropanol/water solvent mixture was prepared and 1cm3 of (CH3)3CCl was added. At specific instances, aliquots of the reaction mixture were withdrawn and quenched with acetone.
A spin vane was added and a water-jacked condenser was attached. Isopentyl nitrite (0.06ml, 0.045 mmol) was dissolved in 1,2-dimethoxyethane (0.50 ml) in a 3-ml conical vial and caped to prevent loss by evaporation. Running the reaction. The mixture in the 5-ml conical vial containing the tetraphenylcyclopentadienone and anthranilic acid was heated on an aluminum block to 140° C. Once the mixture started to boil the prepared mixture of isopentyl nitrite was added to the 5-ml conical vial through the top of the condenser using a pasture pipette.
The purpose of this experiment was to prepare an unknown Grignard reagent and then identify the product by molecular weight and melting point. An IR reading was taken to further identify and validate what product was formed. DISCUSSION AND CONCLUSION Organometallic compounds consist of a carbon that is attached to a metal. The carbon atoms are strongly nucleophilic because of a partial negative charge that they carry.
The objective of this experiment was to use an aldol condensation reaction to synthesize 3-nitrochalcone from 3- nitrobenzaldehyde. This was accomplished with a Diels-Alder reaction that utilized 3-nitrobenzaldehyde, acetophenone, ethanol, and sodium hydroxide. The mechanism for the synthesis of 3-nitrochalcone is presented in Figures 1 and 2. The alpha carbon on the acetophenone is deprotonated. This is followed by the attack of the alpha carbon anion on the carbonyl carbon on the 3-nitrobenzaldehyde.
3. In this experiment, the percent yield was 90%. This number implies that there was little error in this experiment. However, this result could have been caused by certain external factors.
(150.22g/mol)(3.5 x 10^-3 mol of nucleophile) = 0.525 g Actual yield = 0.441 g, Percent Yield = (0.441g/0.525g) x 100% = 84% 10. Percent recovery from recrystallization = (0.172g/0.441g) x 100% = 38% 11.
TrAC Trends in Analytical Chemistry, 22(10), 666-684. Deborde, M., & von Gunten, U. (2008). Reactions of chlorine with inorganic and organic compounds during water treatment—kinetics and mechanisms: a critical review. Water research, 42(1), 13-51. Johnson, J. D., & Jensen, J. N. (1986).
CLAIRE MUNTING 29/01/2018 Criterion C EFFECTS OF SURFACE AREA OF CALCIUM CARBONATE UPON RATE OF REACTION Calcium Carbonate Chips 1 Introduction: Within the current investigation, the effects of the surface area of Calcium Carbonate (CaCO3) in combination with Hydrochloric acid (HCl) upon its rate of reaction. CaCO3, commonly referred to as limestone, is an organic substance and is, in a sense, the crystallised “carbonic salt” of the element, calcium2. In addition to being a salt, the pH level of Calcium Carbonate is 9.91, and it is therefore, a basic substance, due to the fact that it is comprised of a pH level higher than 7, which is neutral3. HCl, however, is the bodily acid found in the stomach of human beings.
The final product weight for percent yield was only the solid E product, which missed one half of the final product produce. If both products were weight, the percent yield would have been larger that it was. Instead of 22.33%, it could have been 44.66%. To prove that both products were obtained, but only one of the two products was analyze, a TLC plate of the DCM layer, that contains both products, and of the final product, was obtain.
Caratonoids have many double bonds in which can undergo isomerisation. In nature they exists in all trans form but under the influence of heat, light or chemical reactions they can
C-H stretch of alkene 2850-3000 2852 C-H stretch of alkane 1705-1720 1710 C = O stretch of acid 1350-1480 1452 -CH bend of alkane 1210-1320 1284 C-O stretch of acid 675-1000 931 = C-H bend of alkene 720-725 721 C-H rock of alkane Figure 5.3 FTIR spectra of erucic