3. Calculate the moles of hydrogen gas collected. (4 points) n = [pic] 4. If magnesium was the limiting reactant in this lab‚ calculate the theoretical yield of the gaseous product. Show all steps of your calculation. (4 points) 5. Determine the percent yield of this reaction‚ showing all steps of your calculation. (3 points) Percent Yield = [pic] × 100 Conclusion: 1. Would the following errors increase‚ decrease‚ or have no effect on the
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Benzoin‚ is provided thereby omitting the first step involving the conversion of benzaldehyde. For this experiment‚ the microscale techniques of reflux‚ crystallization‚ and melting-point determination were used. Utilizing these techniques a product yield of 93% for benzil and 57% for Benzilic acid was obtained‚ as well as a melting point range of 94.8 – 95.4oC for benzil and 152.0 – 153.9oC for Benzilic acid. With the literature melting-point value of benzil being 95oC ( Pavia‚ 2012)‚ the product was
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Formal Lab Report 1 Chemistry 100-03 March 19‚ 2012 Abstract: • Introduction/Objective: Prepare and analyze aspirin from salicylic acid and acetic anhydride‚ and calculate the percent yield of the synthesized aspirin. • Materials and Methods: This experiment called for the synthesis of acetylsalicylic acid‚ or aspirin‚ by using salicylic acid‚ acetic anhydride‚ sulfuric acid‚ and vacuum filtration. The salicylic acid and the acetic anhydride were mixed in a flask. Sulfuric
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must also change from a negative to a positive. The spectator ions were canceled out to yield only the final equations for the reactions‚ specifically reaction 3. The ΔHrxn was calculated by first determining the limiting reactant. The volume was multiplied by the molarity. This gives the value in moles. All the chemical reactions had the same limiting reactant value so therefore they were all equally as limiting. The q values calculated for each reaction were divided by .1 moles. This value was determined
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6 I. Purpose: The purpose of this experiment is to distinguish the relationships between reactants and products‚ in addition to expanding on concepts such as single displacement reactions‚ mole ratio values‚ moles to mass‚ theoretical yields‚ limiting reactants‚ excess‚ stoichiometric relationships and percentage errors. II. Hypothesis: /3 -If the copper metal is submerged in the silver nitrate solution then in reaction‚ a pure‚ solid (Ag) silver product is created with an excess of
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definitions and examples where applicable 1. Product 2. Reactant / Reagent 3. Theoretical Yield 4. Actual Yield 5. Percent Yield 6. Excess Reagent 7. Limiting Reagent 8. Law of Conservation of Matter Short Answer – explain the following: 9. What is conserved in every balanced equation (multiple answers)? 10. What determines the mole ratio in a balanced equation? 11. What is the proper method to determine limiting reagents? 12. What is the relationship between the masses of products and reactants
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were never switched out‚ resulting in one beaker containing alcohol and the ester‚ and not one for each. Because the final product contains ester and alcohol and not just the ester‚ the final weight would be more than it should. This results in a percent yield (95.9%) higher than it should be.
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conducted using semi-microscale recrystallization. The melting point of the product was 136-141 oC‚ which is in the close vicinity of the literature melting point of 146 oC. The theoretical yield of 3-nitrochalcone was 0.253g and the yield after filtration was 0.22g (percent yield of 86.9%). The percent yield after recrystallization‚ was 80.9%. INTRODUCTION The goal of this experiment was the synthesis of 3-nitrochalcone from 3-nitrobenzaldehyde and acetophenone as shown in Figure 1: Figure 1:
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anhydride for the formation of crude acetanilide. The recrystallizing solvent dissolved the crude acetanilide and was heated in a water bath‚ after heating‚ the solution was cooled in an ice bath causing crystals to form. The percent recovery was computed to be 38.49% while the percent yield was computed to be 34.46%. INTRODUCTION Compounds that are obtained from natural sources or from reaction of chemicals almost always contain impurities. The impurities may include some combination of insoluble
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Condensation I.Conclusion Benzoin was produced by reacting 2 mols of benzaldehyde with the catalyst thiamine to form a new C-C bond. A total of 2.626 grams were recovered. There was a 33% recovery of benzoin. The low percent recovery could be due to the purity of the limiting reactant‚ benzaldehyde. Upon filtration‚ the mother liquid appeared oily making it more likely that the low recovery was due to the solution ‘oiling out.’ This could be avoided in the future by maintaining the temperature
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