Yield curve

Discussion The percent yield for this reaction was 8.9%. The theoretical yield for this experiment was 5.95 g, but the actual amount obtained was 0.53 g benzocaine. The percent yield was very low due to inorganic impurities from Na2SO4. These impurities also affected the melting point of the product received. The resulting benzocaine obtained from experimentation had a melting point of 188°C, while the theoretical range for benzocaine is between 121°C-123°C. The sodium sulfate impurities present

reagent phenylmagenisum bromide when reacted with benzaldehyde would be close to theoretical percent yield of 100% was rejected. The measured actual mass was 0.99 g of diphenylmethanol which was relatively low to theoretical mass of 2.708 g of diphenylmethanol. This further concluded to quite low percentage yield of 36.56% of final product diphenylmethanol. As mention earlier, the low percentage yield could be due do many experimental and human errors such as reaction not efficiently reached completion

project. Boston: Harvard Business School Publishing. Krajewski, L.J., Malhotra, M.K., & Ritzman, L.P. (2010). Operations management. Upper Saddle River, NJ: Pearson Publishing. Appendix Figure - Overall Yield, 1973-1977 Figure - Organization Chart

Oetomo, 6 EXPERIMENT 7: OXIDATION OF ISOBORNEOL RAW DATA A & C: MEASURING THE OPTICAL ROTATION OF CAMPHOR SAMPLES AND CAMPHOR OBTAINED FROM OXIDATION OF ISOBORNEOL SAMPLES PATH LENGTH (DM) CONCENTRATION (GR/100 ML) OPTICAL ROTATION (°) #1 #2 #3 AVE Solvent (achiral) 1.97 - -1.5 -1.5 - -1.5 Camphor from camphor tree 1.97 20.83 16.2 16.3 16.3 16.3 Camphor from _Cranensum darlimi_ 1.98 19.65 10.0 9.7 9.8 9.8 Logan's Lumber cat. #3921-5G

Objective The objective of the experiment was to prepare a yield of tert-butylchloride through a unimolecular (SN1) nucleophilic substitution reaction. Procedure Part A- Preparation of tert-Butyl Chloride • A test tube was acquired, and 7 mL of concentrated HCl were added to this test tube through a graduated cylinder, this was done in the fume hood in order to avoid any noxious fumes from the sample, which were observed when pouring in the concentrated HCl. After adding the HCl, a glass pipet

Experiment 4, CHEM 111-520 Introduction In this experiment, metathesis, redox, single displacement, and decomposition reactions were observed and recorded to follow the path of recycled aluminum. The percent yield of the aluminum was also calculated to compare the actual yield with the theoretical yield. The entire concept of aluminum recycling was also observed and successfully reproduced. Materials and Methods The experiment began with the measurement of 0.9300 g of aluminum pieces. The aluminum pieces

Objective The purpose of this experiment was to use stoichiometry to calculate the volume and percent yield of CO₂ produced from a reaction of acetic acid (vinegar) with baking soda. Procedure First the balloon was weighed on its own, and its mass was 2.8 grams. Then the container with the sample of baking soda was weighed and its mass was 14.0 g. The baking soda was then placed into the balloon and the mass was 6.4 g. Lastly, the container minus the baking soda was weighed in order to

Experiment 8: Phenol Alkylation Amber Chavis CHEM 2753 - 007 November 15, 2017 Objective/Purpose: This experiment was designed by conducting a substitution reaction to construct a complex compound (2-methylphenoxyacetic acid) from two simple parts; also known as synthesis - converting simple molecules into more complex molecules. A purification technique known as crystallization was used to purify the product. Suction filtration was used to filter out the product. The experiment was completed over

percent yield obtained for mass was 28.9%. The reason the percent yield was low could be due to the loss of product. This could have happened in several ways including the loss of the organic phase during extraction where too much of the organic phase could have been extracted resulting in less of the product being formed. The lower percent yield may also be due to the reaction not going to completion, resulting in fewer product formed. Additionally, impurities in the product also yield less of the

The collection of excitation and emission spectra provided intensity values that were divided into the intensity of our first solution containing no chloride ions. Our peak wavelengths were consistent and close to the expected wavelengths of 350 nm and 450 nm for excitation and emission, respectively. Our average excitation and emission peak wavelengths were 347.0 (+/-) 1.6 nm and 448.8 (+/-) 2.4 nm, respectively. The peak intensities also decreased in a linear fashion, thus we trusted our spectra