In general, the melt-mixing process induces thermal and thermo-oxidative degradation. Formaldehyde is oxidized to formic acid accelerating the degradation of POM via acidolysis.[4] As mentioned above the addition of bisphenol-A and aniline during the melt-mixing process of POM, allowed the reaction with formaldehyde and generated BA-a and poly(BA-a). At that time, the balance between the formaldehyde consumption to obtain BA-a and the released formaldehyde during thermal degradation of POM is the key point to retard the exposure of formaldehyde to the surroundings. Thermal stability based on formaldehyde releasing temperature and POM degradation temperature is important information to evaluate how an in-situ BA-a formation in POM efficiently …show more content…
The use of TG-FITR was applied so that the degradation temperature and the component generated at that stage can be trace. Figure 3a shows the pristine POM starts showing the formaldehyde peak (CH2O at 1745 cm-1 and 2800 cm-1) at 289 C. As POM-B05A10 was prepared under the condition that POM was molten, the consideration of POM degradation had better reply on the POM after melting, so-called the thermal treated POM, than the pristine POM. Figure 3b shows the thermal treated POM starts to generate formaldehyde at 251C which is much lower than the pristine POM. This implies the ease of formaldehyde generation if the pristine POM was once thermally treated. However, in the case of POM-B05A10, the formaldehyde release is observed at as high as 338 C (Figure 4A) which is 87 C higher than those of POM and thermally treated POM. It is also important to mention that the POM-B05A10 degrades at 431 C which is much higher than that of pristine POM (378 C). This suggests that during in-situ reactive blend of bisphenol-A, aniline, and POM, the formaldehyde released at that melt blend process was effectively entrapped to form …show more content…
The curve fitting analysis of FTIR spectra was carried out. The ring opening of poly(BA-a) could be observed from the disappearance of C-O-C (1233 cm-1). Thus, the integral ratio of the C-O-C (1233 cm-1) over those of the CH stretching (2690 cm-1) was analyzed and shown in Figure S3. It is clear that the poly(BA-a) increases with increasing bisphenol-A content. It might be during the melt-mixing process, by increase in bisphenol-A and aniline content, the formation of BA-a was increased, at that time the oxazine ring-opening polymerization occurred. These lead to increasing
These tests were the silver nitrate test and the sodium iodide test. The goal of these tests was to verify that 1-bromobutane, a primary alkyl halide, had in fact been formed. Data and Results 0.844 grams of product were collected. As 1-bromobutane has a molecular weight of 137.02 grams/mole, this gives 0.00616 moles of 1-bromobutane. The limiting reagent in this reaction
Purpose: To ascertain the decomposition reaction of baking soda using stoichiometry. The purpose is also to find the correct equation for the reaction. Hypothesis: The chemical equation for the decomposition of baking soda is sodium bicarbonate (s) → sodium carbonate (s) + carbon dioxide (g) + water (g)
Chem 51LB Report Ngoc Tran - Student ID # 72048507 The purpose of this lab is to examine the composition of three components of gas products of elimination reaction under acidic condition by conducting the dehydration of primary and secondary alcohol, and under basic condition by conducting the base-induced dehydrobromination of 1-bromobutane and 2-bromobutane. Then gas chromatography is used to analyze the composition of the product mixtures. Gas chromatography (mobile phase) is used to analyze the composition of three components of the gas products. A syringe needle with gas product is injected into the machine, and the component is eluted and the composition is related to the column or the peaks.
The crude tetraphenylnaphthalene in a 25-ml Erlenmeyer flask and dissolved in boiling isopropyl alcohol (12 ml). The solution was cooled to room temperature and further cooled in an ice bath for 30 minutes. Crystallization of colorless crystals occurred. The product was collect in a Hirsch funnel and washed with isopropyl alcohol. The solid was left to dry over the weekend.
In the round-bottom flask (100 mL), we placed p-aminobenzoic acid (1.2 g) and ethanol (12 mL). We swirled the mixture until the solid dissolved completely. We used Pasteur pipet to add concentrated sulfuric acid (1.0 mL) to the flask. We added boiling stone and assembled the reflux. Then, we did reflux for 75 minutes.
9. The melting point range was lower than the given range of the anti-addition product by 2 degrees Celsius. This could have been due to impurities in the product. A likely cause could have been water that still remained in the product after recrystallization (the product shifted upward during melting point analysis due to evaporation). Since water has a low melting point, it could have lowered the melting point range of the product.
Experiment 3 comprised three reactions: formation of dimethyl tetraphenylphthalate, hexaphenylbenzene, and tetraphenylnaphthalene. All 3 reactions used tetraphenylcyclopentadienone as the diene to generate products with high aromatic stabilization. The first reaction was the formation of dimethyl tetraphenylphthalate. A cloudy white solid was formed with 31.1% yield.
The decomposition of NaHCO3 is an example of Prevention within Green Chemistry principles because all solid waste in this experiment is collected and used again. The only gaseous wastes generated by the reaction in the experiment are carbon dioxide and water, which are benign (Lab 3). The decomposition reaction of NaHCO3, generates virtually no waste, therefore less hazardous chemical syntheses. The byproducts of the reaction are gaseous CO2 and H2O which possess little or no toxicity to human health and the environment, because of the amounts released in this experiment. (Lab 3).
The results were an indicative for expected IR spectrum of pure phenacetin. The IR spectrum showed peaks at (3281.67 cm-1) which indicate the presence of the N=H stretch, (3131.40 cm-1 and 3073.97 cm-1) representing the Sp2 C-H stretches, (2982.26 cm-1, 2927.60 cm-1 and 2885.53 cm-1) expressing the Sp3 C-H stretches, also (1656.82 cm-1) indicating the C =O amide stretch, and finally a wavelength at (1603.51 cm-1) representing the aromatic C =C stretch of the phenacetin molecule, respectively. Such IR spectrum results from phenacetin in comparison with an acetaminophen IR spectrum clearly showed the elimination of the hydroxide (OH) bond present at the acetaminophen molecular structure, which resulted in the IR spectrum not indicating the presence of a strong and broad (alcohol-phenol) band at about 3500 cm-1
The triphenymethanol product was a very fine white powder that had a slight yellow tint to it. The experimental melting point was calculated to be 159.0-159.6°C, which is very accurate compared to the actual melting range of 160-163°C. The percent yield came out to be 26.89%, which is most likely low due to using heating plates to heat the end reaction instead of the recommended steam baths. 2. N/A 3.
The possible explanations and changes to make are similar to the previous questions. Conclusion and Future Experiment 18. The identity of the product and unknown were 4-tert-butylbenzyl phenol ether and tert-butyl phenol respectively. The key to making this discovery was the melting point and TLC results!
This was proved by utilizing the IR spectrum to verify the C =O was not in the final product as it lacked the 1640 cm-1 peak. The melting point of 113-115 degrees C proved that the final product obtained was the E-Stilbene. The TLC plate proved that the E and the Z product was produced, show cased by the double intensity of the DCM spot to the final product’s spot, both which had an Rf of 0.92. The double intensity proved that both products were produced, but through heating and filtering, the Z-Stilbene was
In this experiment, it was possible to produce the major products from bromination of acetanilide and aniline. 0.075g of 4-bromoacetanilide and 0.156g of 2,4,6-tribromoanilne were collected from bromination of 0.07g acetanilide and 0.05g aniline with the percent yield of 67.57% and 88.1% respectively. At the end of the experiment, to prove the formation of the major products, melting point of the products were measured. The melting point of the product from the bromination of acetanilide was 164.8-168.50c, which is in the range of the melting point of 4-bromoacetanilide, 165-1690c, as reported on the Chemical Book, CAS Database List (chemicalbook.com). The melting point of the product from the bromination of aniline was 119.8-121.90c, which is in the range of the melting point of 2,4,6-tribromoaniline, 120-1220c, as indicated on PubChem, Open Chemistry Database (pubchem.ncbi.nlm.nih.gov).
Purpose/Introduction The process of recrystallization is an important method of purifying a solid organic substance using a hot solution as a solvent. This method will allow the separation of impurities. We will analyze Benzoic Acid as it is dissolved and recrystallized in water and in a solvent of Methanol and water. Reaction/Summary
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.