Yield curve

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

ether was used to wash the crystals on the watch glass and was removed using a pipet. Results With the methods used, .053g of 4-Methoxyacetophenone was obtained. Discussion The theoretical yield of 4-Methoxyacetophenone is .764g. Our actual experimental yield was .053g. The percent yield was 6.9%.

15 (g/mol) = 0.00925 moles Using 1:1 stoichiometric ratio for product theoretical yield estimation: 0.00925 moles x MW of chloride (35.45) = 0.328 grams of product Percent Yield = Actual yield / theoretical x 100% = 0.228 (g) / 0.328 (g) x 100% = 69.51 % Discussion It is not uncommon to have a percent yield less than 100% as was observed in our experiment. Imperfect percent yield can be interpreted that the condition were not optimal and could be improved. Despite

period. The percentage yield was calculated to be 17% and the melting point rangeof the product obtained was 100.8C-104.8C. Procedure: The procedure for this experiment is found in the organic chemistry I lab manual written by Zachary Poulos (pages 123-134). There were no changes to the procedure. Reaction Data and calculations: Data: Original Mass of Cholesterol (mg) 102 mg Mass of empty Al dish (mg) 405 mg Mass of Al dish & Cholesterol dibromide (mg) 429 mg Percentage Yield (%) 16% Melting point

This was calculated by taking the mass of 4-tert¬-butylcyclohaxanol, dividing it by the theoretical yield determined by mass of the limiting reagent, 4-tert¬-butylcyclohaxanone, and multiplying by 100. This percent yield is respectable, but a higher one could have been obtained. A source of error resulting in a lower percent yield was the filtering to remove the magnesium sulfate out of the dried organic solution. When filtering, some of the liquid was absorbed into

The objective of the lab is to recognize the importance of observation in the scientific method, merely applying the copper cycle and the process and reactions that take place throughout. Copper is present in several biological systems, having both biological and environmental implication. Sets of experiments will alter copper into nitrate salt, then a hydroxide, followed by an oxide and sulfate, before reaching the state of metallic copper once. These reactions are managed to test the copper in

Percent yield is determined by calculating the theoretical and actual masses. The theoretical yield is the expected or maximum amount of product you should see in a reaction8. Ideally, the percent yield should be one hundred. The results of the percent yield calculations are indicated in Table 5. For the two detergents, the percent yields were lower than one hundred. This could have occurred because of many different errors during the experiment. One of those errors could have been that some of the