Theoretical Yield Lab Report
1. What was your theoretical yield and your percent yield? Theoretical yield: 3.9151 g Percent yield: 79.30% 2. An accurate percent yield must be below 100% Why? (2-3 sentences) First, percent yield cannot be over 100% because mass cannot be created; the collected mass of a substance can never go over the theoretical yield of that substance. Percent yield is also very rarely 100% because no equilibrium reaction, which is the type of reaction studied in this lab, can go to completion. There is always some amount of products that transforms back into reactants; therefore, theoretical yield, which assumes that the reaction goes to completion, will rarely equal experimental yield. 3. What error(s) may have caused a percent yield higher than
Chem 100 Final Lab Report
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Triphenylmethyl Bromide Lab Report
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840 Words | 4 PagesAs 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.
Stoichiometry Lab
563 Words | 3 Pages3. 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.
Copper Recovery Lab Report
471 Words | 2 PagesThe percent recovery of the copper was calculated using the equation, percent recovery = (the mass of the copper recovered after all the chemical reactions/the initial mass of the copper) x 100. The amount of copper that was recovered was 0.32 grams and the initial mass of the copper was 0.46 grams. Using the equation, (0.32 grams/0.46 grams) x 100 equaled 69.56%. The amount of copper recovered was slightly over two-thirds of the initial amount.
Nucleophilic Substitution Reactions Lab
1039 Words | 5 Pages(150.22g/mol)(3.5 x 10^-3 mol of nucleophile) = 0.525 g Actual yield = 0.441 g, Percent Yield = (0.441g/0.525g) x 100% = 84% 10. Percent recovery from recrystallization = (0.172g/0.441g) x 100% = 38% 11.
Photosynthesis Lab Report
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Wittig Reaction Lab Report
1125 Words | 5 PagesThe final product weight for percent yield was only the solid E product, which missed one half of the final product produce. If both products were weight, the percent yield would have been larger that it was. Instead of 22.33%, it could have been 44.66%. To prove that both products were obtained, but only one of the two products was analyze, a TLC plate of the DCM layer, that contains both products, and of the final product, was obtain.
Stoichiometry And Limiting Reagents Lab Report
1237 Words | 5 PagesThe actual data is the result on our experiment vs theoretical, which is based on the calculations above. I have also learned to pay more attention to draining out all of the product completely before continuing to test the experiment, as any small drop of contaminant can veer our results into a different
Exponential Growth Lab Report
513 Words | 3 PagesExponential Growth of E. coli Escherichia coli, also more commonly known by the name E.coli, is a commonly found in the large intestines of warm-blooded organisms. The strains of bacteria that are found in the body are not harmful and can actually aid the body in things like digestion. E.coli, like a lot of bacteria, have a growth stage that can be expressed exponentially in both an equation and on a graph. In order to calculate and predict the number of E. coli bacteria cells growing on a plate of medium after a certain amount of time, an equation for continuous exponential growth can be created using the formula A=Pe^rt, in which A represents the ending amount of bacteria, P represents the number of bacterial cells initially on the plate,
What Happens When Can Yeast Metabolize?
451 Words | 2 PagesFor example, in the response experiment, a yeast solution was prepared without sugar mistakenly and thus had to be prepared again. This suggests that other errors in preparation and measurement could have been encountered. For the future, careful measurements using clean uncontaminated flasks would eliminate possibilities of such error. A source of error for the metabolism experiment involves the yeast’s yellow hue. It is possible that the color of the yeast caused the solution to look more
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