Earnings yield

It’s actually a very simple quantitative stock ranking scheme. It uses return on capital and earnings yield as inputs. Return on capital is the metric that shows whether a business is a good one or not. Earnings yield is the metric that shows whether a company is cheap or not. Greenblatt suggests using these measures to identify good but cheap businesses, and buy them. That’s the secret behind the ‘magic

the most recent month. After learning about the post earnings announcement drift, you decide to give it a try. You gather most recent earnings information on 100 stocks as of April 30 2013. After examining the earnings surprises, you decide to buy an equally weighted portfolio of the top 10 stocks with the most positive earnings surprises. At the same time,

The objective of the experiment was to synthesize a sample of cyclohexene by using an E1 reaction, which involved cyclohexanol. Procedure Part A- Preparation of Cyclohexene • Prior to beginning the procedure, a distillation setup was constructed in order to prepare for a later step in the procedure; a diagram of the construction was included in Figure 1.A. In a clean 50-mL Erlenmeyer flask, 5 mL of water were placed, and, with extreme caution, 4.0 mL (8.0 g, 0.08 mol) of concentrated sulfuric acid

and a polymer-supported reaction. II. Reaction Equations and Mechanisms III. Calculations Part 1 Theoretical Yield 1) (1.62 g ethyl vanillin x 154.16 g ethyl vanillyl alcohol) / (166.18 g ethyl vanillin) = 1.503 g ethyl vanillyl alcohol 2) (0.3 g NaBH4 x 154.16 g ethyl vanillyl alcohol) / (37.83 g NaBH4) = 1.223 g ethyl vanillyl alcohol Percent Yield = (1.03 g / 1.223 g) x 100 = 84.2% Melting Point Range ( ̊C): 83.9, 84.4, 85.0 Melting Point Average ( ̊C): 84.43 Rf

In this experiment, a Fischer Esterification reaction was performed with two unknown compounds. The unknown compounds, Acid 2 and Alcohol D, were identified by using the knowledge of the reaction that took place, and the identity of the product that was synthesized. The identification of the product resulted from analysis of IR and NMR spectra. For this experiment, Alcohol D and Acid 2 reacted in the presence of concentrated sulfuric acid, resulting in a colorless solution with brown layer on top

found in figure 1.0 was 0.0978mg/mL. Presumably, the mass (in mg) of pure ASA based on the two consecutive dilutions was approximately 97.8 mg this value is unsuccessfully proven to match the associated theoretical value due to the overall percent yield, which will be discussed further. Also, according to the same calculations made in calculation #1, the calculated mass for Bayer Aspirin was inaccurate as the calculated value was less than what was said by the company. In other words, the Bayer Aspirin

of Na2CO3 was reacted with a solution of CaCl2 to form a precipitate of CaCO3. The theoretical yield of CaCO3 was calculated and then compared to the actual yield of CaCO3. The results suggest that the Theoretical Yield was 4.2246 grams and the Actual Yield was 4.24 grams, which gave a Percent Yield of 100.473% and a Percent Error of 0.473%. The actual yield was greater than the theoretical yield. It is suggested that it was greater than because I used two different filter papers and I only

crude product was collected by crystallization process, it was weighted to be 8.4756 g. it was recrystallized and collected. The weight of pure product was obtained to be 5.772 g In comparison to the theoretical yield of the experiment; it was calculated to be 65.99 % recover and 82% total yield. The melting point (MP) of the product was taken in order to identify the product. 2 trials were performed, and the results of both trials are the same, 102-105oC. The expected product of this experiment was

Examining the Percentage Yield of a Chemical Reaction Komal Maan 470883 Ms. Chandan April 28th, 2015   Introduction: Numerous factors can determine the percentage yield of a chemical reaction. Such as the nature of the reaction, the conditions in which the reaction is carried out and the nature of the reactants used in the reaction. In this investigation the percentage yield was to be determined using the following chemical reaction: Fe(s) + CuCl₂ (aq) FeCl₂ (aq) +Cu(s) Steel wool was used

In order to calculate the percent yield, we first had to determine the moles of the limiting reactant, which was anthranilic acid in this case, by dividing the mass of was anthranilic acid we weighted in the beginning of the lab (2.001g) and dividing it with the molar mass of was anthranilic acid. Thus obtaining the value of 0.01456g. Then in order to calculate the theoretical yield, we multiplied the moles of was anthranilic acid with the molar mass of N-acetylanthranilic acid and the mole ration