Abstract: Cyclohexanone a cyclic ketone was oxidized to adipic acid using the oxidizing agents concentrated nitric acid. Then, the recrystallized product was characterize by using infrared spectroscopy and taking the melting points. The experiment yielded 0.199 grams of adipic acid and a very high percent yield of 106.40%. Upon examination of IR-spectrum, Adipic acid was identified by comparing it to the IR-spectrums provided in the lab book. Furthermore, the melting point of the experiment was obtained to be 151-154 ºC, which included the theoretical melting point of 153 ºC between the experimental melting point range. Introduction: Redox reactions are very important in organic chemistry and they involve transfer of electrons from one molecule to another. Oxidation occurs when a carbon atom becomes bonded to a more electronegative atom, causing the electron density on carbon atom to decrease (McMurray, 2012). That was the part that our experiment focused. The oxidation of Cyclohexanone for the …show more content…
One small drop of Cyclohexanone from a vial containing 150 mg of ketone. The tube was warmed on a sand bath until the brown oxides of nitrogen are emanating from the nitric acid. The solution was allowed to boil until it was almost clear. Then the tube was removed and the Cyclohexanone was added drop by drop within a time period of about one minute and it was allowed to boil again until it turned clear. The tube was then allowed to cool at room temperature and fine crystals were observed. The tube was cooled in an ice bath for about 3 minutes and the crystals were stirred with the tip of Pasteur pipette and the solvent was removed from the crystals. 0.2 mL of ice cold water was added to crystals and then the solvent was removed again using a Pasteur pipet. Once most of the solvent was removed, the crystals were spread on a filter paper and allowed to dry for next
In this lab, the oxidation of a secondary alcohol was performed and analyzed. An environmentally friendly reagent, sodium hypochlorite, was used to oxidize the alcohol, and an IR spectrum was obtained in order to identify the starting compound and final product. The starting compound could have been one of four alcohols, cyclopentanol, cyclohexanol, 3-heptanol, or 2-heptanol. Since these were the only four initial compounds, the ketone obtained at the end of the experiment could only be one of four products, cyclopentanone, cyclohexanone, 3-heptanone, or 2-heptanone. In order to retrieve one of these ketones, first 1.75g of unknown D was obtained.
K.D.A. Saboia et al. , (2007) have been prepared the Bi4Ti3O12–CaCu3Ti4O12 {[BIT(X)–CCTO(100-X)]} composite powders through solid state reaction method and calcined in the range of 900 to 1020 ºC for 12 h. The as-prepared powders have modified in the form of thick film onto alumina ceramic substrate by utilizing screen printing. At 100 Hz, the value of dielectric constant (κ) of CCTO100 and BIT100 is 316.61 and 53.64 respectively. Conversely, the composite with X=20 % shows an unexpected dielectric constant of 409.71, which is around 20% higher in comparison with the CCTO.
Procedure and Observations To begin the lab, first all the correct equipment and materials had to be collected
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.
Use a spatula to scoop and place 2 crystals of CuSO4●5H2O into a test tube. 2. Describe the crystals. 3. Light a Bunsen burner.
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.
After the assigned reaction was complete, samples of authentic cis-cyclohexene-1,2-diol, authentic trans-cyclohexene-1,2-diol, a 50:50 mix of the cis and trans cyclohexene-1,2-diols, and the product were each spotted on the Thin Layer Chromatography (TLC) plate. Then the TLC plate was placed inside a saturated beaker filled ethyl acetate in order to develop the plate. Once the solvent traveled up the solvent front, the plate was stained with anisaldehyde solution and then heated with a heat gun so the results could be visible. When looking at the results, the spot for the authentic cis-cyclohexene-1,2-diol turned a dark purple/light pink color, the spot for the authentic trans-cyclohexene-1,2-diol turned a light purple/blue color, the spot of the 50:50 mix of the cis and trans cyclohexene-1,2-diols turned a dark purple/light pink color, and the spot for the product turned a dark pink color. The color similarities between the product, the cis-cyclohexene-1,2-diol, and even the 50:50 mix of cis and trans diols indicated that the
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.
Glacial acetic acid and acetic anhydride were added to the mixture while refluxing, which converted the lime colored solution into a clear mixture. The flask was cooled in an ice bath and the solution
Weighed 1 gram of NaC2H3O2 and mixed it with ionized water. Boiled 12 mL of 1.0M Acetic Acid added into a beaker containing the sodium carbonate on a hot plate until all the liquid is evaporated
Name :SiphesihleGamede Student number : 213571124 Experiment : #10 Date : 4 March 2015 Experiment Name : High Performance Liquid Chromatography (HPLC), Quantification of caffeine in various drinks Aim The aim of this experiment was to ascertain the concentration levels of caffeine in cola soft drink samples such as coke, monster and red bull by utilising the internal standard method using HPLC. The experiment was also aimed at investigating the use of solid phase extraction for sample clean-up.
(NH4)2CO3 was added to the solution. Then the tube was placed into warm water. Once the tube was cooled, the tube was centrifuged and 0.5 mL of 6M acetic acid was added to the precipitate. This was done to see if the precipitate turned cloudy. The solution was clear and not cloudy.
Introduction Chevron Phillips Chemical Company is the major producer of Cyclohexane. This successful company hoses the three largest cyclohexane plants in the world. Many are puzzled by how the production of cyclohexane seems to have become stagnant. Perhaps this is due to the cost of benzene increasing or the demand increasing. Through thorough investigation, the answer to this question and many more can be answered.
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.