Exercise 2: a. 0.43 g of ZnI2 B 5E-4 moles of ZnI2 c. 0.161M* x L=moles of ZnI2 in solution 84 mL for the first student 31 mL for the second student 3. Exercise 3: a. 2.56 g/500 mL (given) b. 0.00512 * 500 = 2.56 c. 0.00806 * 319.9= 2.56 d. 0.00806 * 319.9 = 2.56 500 mL =0.5 L e. 0.0161 * 500 / 2 =2.56 4.
Synthesis of Methyl Stearate Post-Lab Submitted by Matthew Sharma TA: Evan Determining the Limiting Reagent Methyl Oleate (MW= 296.49 g/mol) Amount used = 1.141g (1.141g)(1mol / 296.49g) = 0.003848 mol ∴ The limiting reagent for the reaction is methyl oleate because hydrogen is used in excess Theoretical Yield Methyl Stearate (0.003848 mol)(298.504g/mol product) = 1.1486 g methyl stearate Percent Yield Given the 1:1 stoichiometry of the reaction: 100% x (0.2551g product / 1.1486g theoretical yield) = 22.2% Conclusion A 22.2% yield of synthesized methyl stearate was obtained via the catalytic hydrogenation of methyl oleate in the presence of the catalyst 10% palladium on carbon. The product
Some of the black precipitate becomes stuck to the side of the beaker as it’s being stirred and some of the liquid being vaporized. By decanting the solution, much of what is left in the beaker remains black precipitate; however, some clear liquid can also be seen. A slight loss of black precipitate was also observed from decanting. The precipitate completely dissolves with the addition of roughly 25 drops of HCL and there is a change of color to yellow-green. As the drops are being added, a distinct yellow color can be observed where the drops were landing in the solution.
Powder B, when water was added, it only became watery. When vinegar was added, the liquid sunk to the bottom and none of the outcomes changed. With iodine, it had a color change with some bubbles but shortly after it went back and stayed the color brown. Powder C, it was not affected by water but by vinegar, it changes into bubbles and fizzes up and has a chemical reaction. With iodine it changes to a brown color and becomes clumpy.
Juliana Park Mayumi Tamada CHEM 111B LAB/ M-F 1-4PM 15 August 2012 Spectroscopy Lab Introduction In this lab, the molar absorptivity of the complex FeLn2+ will be determined by using the absorbance of the complex and its concentration. The absorbance will be found by using a spectrophotometer. For the next part of the lab, the formula of the complex will be determined by also using the volume of ligand and the absorbance again. Experimental There are two different parts to the experiement. In the first part, five 100 mL flasks of 5 mL ligand solution, 5 mL 2 M sodium acetate, 4 mL 3 M NH2OH, and 1-5 mL Fe2+ solution are diluted with water.
0.0625mol/0.125M=0.5L=500mL Calculation for preparing the EDTA solution Exercise 6 a. 1L*0.02M=0.02mol 0.02mol*372.24g/mol=7.4g EDTA b. Exact molarity of 7.4448g /1.00L would be .0200 M Exercise 7 a. 0.5M*100*10-3L=0.05mol acetic acid b. 0.05mol/6M=8.3*10-3 L=8.3mL stock solution c. 100mL-8.3mL=91.7mLwater Add 91.7 water to 6M stock solution to prepare 0.5M acetic acid.
ABSTRACT Isopropyltoluene isomers were synthesized through the friedel-crafts alkylation of toluene with 2-chloropropane in the presence of aluminum chloride as a catalyst. Through extraction of the distillate with water and 5% NaHCO3, followed by a fractional vacuum distillation, the desired aromatic organic compound was isolated. Infrared Spectroscopy and Gas Chromatography were used to analyze the composition, purity and to confirm the identity of the prepared product. The sample weighed approximately 2.66g, which reflected a low yield at 47%. However, from the GC the area % (also known as percent purity) was 91.8%, which indicates that a very pure product was obtained.
Predict the number of valence electrons for a sulfur atom. a. 4 b. 6 c. 8 d. 16 e. 32 58. Predict the number of valence electrons for a chlorine atom.
The bromine is acting first like an electrophile, and then after bromine has broken the π bond, a carbocation has formed, and a bromide ion has been created, the bromide ion then acts as the nucleophile and forms a bond with the carbocation. This experiment uses bromination, the specific name of halogenation with bromine. In order to for bromination to occur bromine must first be generated. This is done in situ through the oxidation of glacid acetic acid and puridinum bromide perbromide. Once generation is accomplished the available bromine can be brominated.
2. What would happen to the water if instead of coffee beans, strips of dried seaweed were used? Explain your prediction. Since the dried seaweed is not as soluble as the coffee beans, a solution of seaweed and water would not form. Rather, overtime the dried seaweed would soften with the water and form a mixture.