questions: 6) If I do this reaction with 35 grams of C6H10 and 45 grams of oxygen‚ how many grams of carbon dioxide will be formed? 7) If 35 grams of carbon dioxide are actually formed from the reaction in problem 6‚ what is the percent yield of this reaction? Exam Review Sheet #1 Balancing Equations and Simple Stoichiometry Answers are provided on the second sheet. Please try to do the worksheet without referring to them‚ because you’ll be expected to know
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Final Organic Study Guide: Be able to develop an Experiment Beginning to End * Find a good reaction * Good reaction is defined by high yield‚ green chemistry (less waste‚ less harmful chemicals) * Reaction found on Reaxys * Find MSDS Sheet for all Compounds (Reactants‚ Products and Side Products) * It is important to know what you are working with * The toxicity category numbers are there to gauge how toxic the chemical is‚ 4 being most severe and 1 being least
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to its secondary alcohol product via reduction reaction. This two-step reaction reduces aldehydes by hydrides to primary alcohols‚ and ketones to secondary alcohols. In order for the reaction to occur and to better control the stereochemistry and yield of the product‚ the metal hydride nucleophile of the reducing agents such as LiH‚ LiAlH4‚ or NaBH4 must be carefully chosen. Being that LiAlH4 and NaBH4 will not react with isolated carbon-carbon double bonds nor the double bonds from aromatic rings;
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Background 1 2 Theory 1 3 Procedure 2 3.1 Materials 2 3.2 Preparation 2 3.3 Recrystallisation 3 3.4 Determination of Melting Point 3 4 Results and Calculation 4 4.1 Mass 4 4.2 Percent yield 4 4.3 Melting Point 4 4.4 Appearance 4 5 Discussion 5 6 Conclusion 5 References R1 Synopsis This report is based on preparation and recrystallization of aspirin. The objective of the experiment
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the percentage yield in order to see the amounts of anhydrous sodium carbonate and calcium chloride were used up. Also to see if there’s any alterations like mass differentials. Objectives: 1. To introduce the concept of “limiting factor” in a chemical reaction 2. To practice a. Writing a balanced equation b. Determining the number of moles of each reactant and product c. Deciding which chemical is the limiting factor d. Predict theoretical yield e. Determine
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Williamson Ether Synthesis specializing in producing ethers‚ it was ideal for this lab because of the alcohol and the alkyl halide used. After the synthesis and isolation of Gauifenesin was completed‚ the melting point ranges were observed and percentage yields were calculated to compare with the values of authentic guaifenesin and guaiacol. Reflux was used to synthesize Guaifenesin. Guaifenesin is an expectorant‚ meaning it helps loosen congestion in one’s chest and throat‚ making it easier to cough
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the compounds used in that lab. In such a case‚ also replace “Yield Calculations” with a “Percent Composition” of what you were analyzing/separating. Yield Calculations: [pic] [pic] Because there are less moles of sodium benzoate‚ it is the limiting reagent. [pic] The theoretical yield of Benzoic Acid is 1.695 g. The actual yield of Benzoic Acid is : whatever you got in your experiment. The percent yield of this experiment is: [pic] ***Note that for this section
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by the smallest number mole to reduce the decimals 3) If not whole numbers yet‚ multiply by some special factors to reduce decimals 1.25 x ¼ = 1 Al2(SO4)3 + 3 Cu : 2:3:1:3 ratio To determine amounts‚ use ratio and plug in numbers correctly Limiting/excess reactants Limiting:Reactants that are not completely used up in a reaction When this reactant is used up‚ the reaction stops Excess
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C6H5COOH(s) + NaCl(aq) Upon completion of this experiment students will gain experience using common extraction techniques such as vacuum filtration‚ as well as familiarity with common calculations used in chemistry‚ such as mass measurements and percent yield. Description of Procedure: 2.00 g of sodium benzoate was dissolved in 10.0 mL of H2O. 7.0 mL of HCl was added to the solution and a pH of 2 (similar to stomach acid) was reached. Upon addition of the HCl‚ a white precipitate formed. The mixture
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Lab 3: Stoichiometry of a Precipitation Reaction NOTE: All photos should be taken so the reading on the electronic balance is readable. Photo 1: filter paper being weighed on electronic balance‚ along with your student information card. Photo 2: beaker with precipitate slurry in it (after step 5) ‚ along with your student information card Photo 3: dried precipitate/filter paper being weighed on electronic balance‚ along with your student information card Additional Question Guidelines:
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