Isopentyl acetate was prepared by fluxing it with alcohol with also some mixture of acetic acid and hydrochloric acid. The acetate was obtained by distillation method with 0.41g and a percent yield of 20%. The mass obtained in this experiment was approximately two times lower compare to the mass in the lab manual book. This might occur during the extraction of the aqueous solution in each step of the experiment. Due to the low of the mass of isopentyl acetate, the percentage yield (20%) was like three or 4 times lower than the normal percent yield of the product. Even though we had a strong smell of banana, but there was the presence smell of some other compounds as the NMR spectrum shows (see attach sheet). This showed that the product obtained was not completely pure due to the extraction or distillation process, but not to forget that it can also be due to the unclean of materials. The NMR data was consistent with the one expected for the product, where the CH bond was deshield, and the CO bond the shield, but not the least shield (see attach sheet). Conclusion …show more content…
In this experiment, (mass of isopentyl acetate) was formed directly by esterification of acetate acid with isopentyl alcohol. Sulfuric acid was used as a catalyst. The percentage yield of isopentyl acetate was approximately 20% with a theoretical of 2.082g. This might due to the reason that I lost some of my product in the distillation process. It also might be the fact that my TF told me to add a little drop of sodium chloride in the solution because it was cloudy right after I added 5ml of water. Another error might include using unclean glassware. This experiment was partially success since the reaction produced a banana smell despite the low percent yield
After adding the acetic acid and hydrobromic acid to the solution, and heating and recrystallizing the solution, the product triphenylmethyl bromide was created and had a mass of 0.103 g. The theoretical yield was calculated by determining the limiting reagent in the reaction. The triphenylmethanol was the limiting reagent in the reaction. The total amount of mass from the triphenylmethanol was converted to moles by using the molar mass of the triphenylmethanol. The amount of moles was then converted into grams to determine the theoretical yield, 0.125 g. The percent yield was then calculated by dividing the actual yield by the theoretical yield and multiplying the result by 100%. The percent yield was 82.4%.
The last goal was to determine the percent yield of a product formed during a reaction with the unknown compound. Experimental Design The first day of lab consisted of various preliminary tests that helped identify the unknown compound.
After obtaining an homogeneous mixture, the flask was placed in an ice bath during five minutes next to a graduated cylinder containing 5.0 mL of concentrated sulfuric acid. The temperature of the ice bath was recorded to be 1.1 °C. Likewise, a second graduated cylinder containing 1.8 mL of nitric acid and 2.5 mL of sulfuric acid was immersed in the cold ice bath to keep the three different solutions at the same temperature. Thereafter, the cold 5.0 mL of H2SO4 were added to the erlenmeyer flask containing the acetanilide solution, which remained in the cold water for approximately another 4 minutes.
Dehydration of 2-Methylcyclohexanol Sura Abedali Wednesday 2:00 PM January 31, 2018 Introduction: Dehydration reactions are important processes to convert alcohols into alkenes. It is a type of elimination reaction that removes an “-OH” group from one carbon molecule and a hydrogen from a neighboring carbon, thus releasing them as a water molecule (H2O) and forming a pi bond between the two carbons1. In this experiment, 2-methylcyclohexanol undergoes dehydration to form three possible products: methylenecylcohexane, 1-methylcyclohexene, and 3-methylcyclohexene in a Hickman still apparatus. Adding 85% Phosphoric Acid to protonates the “-OH” group, turning it into a better leaving group and initiating the dehydration reaction.
Lab Report 5: Acetylsalicylic Acid (Aspirin) Synthesis Name: Divya Mehta Student #: 139006548 Date Conducted: November 19th 2014 Date Submitted: November 26th 2014 Partner’s Name: Kirsten Matthews Lab Section: Wednesday 2:30 L9 IAs Name: Brittany Doerr Procedure: For the procedure, see lab manual (CH110 Lab Manual, Fall 2014) pages 96-98. Wilfrid Laurier University Chemistry Department. Fall 2014. Acetylsalicylic Acid (Aspirin) Synthesis.
As seen in table 1, the theoretical yield was .712 g of C_17 H_19 NO_3. The % yield of this experiment was 7.51 % of C_17 H_19 NO_3. . This low yield can be explained from a poor recrystallization technique combined with potential contamination. Throughout the experiment, the mixture changed color from green, orange, to yellowish lime, and eventually clear.
To determine the rate of reaction there are many method to be used for example, measuring the mass after the product has been added and measuring the difference in mass on the duration of a digital scale. Another method, which will be used in this experiment is using a gas syringe to measure the volume of the gas which has been produced. The cylinder inside, will be pushed out to show a quantitative presentation of the volume produced by the reaction. Hypothesis
Leah Romero 10/30/2017 Conclusion Lab 3 Chem 102L In lab 3, fundamentals of chromatography, the purpose was to examine how components of mixtures can be separated by taking advantage of different in physical properties. A huge process in this lab was paper chromatography, which was used to isolate food dyes that are found in different drink mixes. The different chromatograms of FD&C dyes were compared to identify which dyes are present in each of the mixes.
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.
Experiment 2 Report Scaffold (Substitution Reactions, Purification, and Identification) Purpose/Introduction 1. A Sn2 reaction was conducted; this involved benzyl bromide, sodium hydroxide, an unknown compound and ethanol through reflux technique, mel-temp recordings, recrystallization, and analysis of TLC plates. 2. There was one unknown compound in the reaction that was later discovered after a series of techniques described above.
This supports the isolated product is majority made of the desired product and is largely pure. Mass spectrometry of the crude product shows the molecular ion peak is 162.1, which is the largest fragment in the mass spectrum (Figure 4) and corresponds to the molecular weight of methyl trans-cinnamate (Table 1). The base peak is 131, inferring the fragment lost is 31 m/z in size. This 31 m/z matches the OCH3 fragment of the ester, and would not result from a trans-cinnamic acid. This is evidence the product was successfully
The percent yield was 22.33%. In most cases, that means that a lot of possible product was lost. However, in this case, that was not true. When Benzaldehyde reacted with the Wittig reagent, it produced two products: E-Stilbene and Z-Stilbene. The Z product was a liquid, while the E product was a solid.
Then percent yield was calculated to be 67.57%. The isolation of less product resulted from using less amount of acetanilide than 0.07g at the beginning of the experiment. In addition, the melting point of the product was measured to be 164.8-168.50c, which is in the range of the normal melting point of 4-bromoacentailide, 165-1690c. This confirmed the formation of 4-bromoacetanilide from the bromination of acetanilide. From the bromination of 0.05g aniline, 0.156g of the product was collected.
Purpose The aim of this experiment is to an amide is created by treating an amine with acid anhydride during acetaminophen preparation. Acetaminophen (p-acetamidophenol), the amide, is produced when the amine p-aminophenol is subjected to treatment by acetic anhydride. Experiment Data/Results
14- Determine the yield, refractive index, and % yield of ester. Conditions :- 1) This reaction is catalyzed by acid, Like Fischer esterification. 2) Usage of water in step (5):So that after Estrification is completed , any excess unreacted acetic anhydride is hydrolyzed. 3)