225 g Moles of Ferrocene 1.21 * 10 ^ -3 mol Initial volume of acetic anhydride 1.00 mL Moles of acetic anhydride 0.0110 mol Initial volume of phosphoric acid 0.300 mL Initial moles of phosphoric acid 5.15*10^-3 mol Limiting reagent Ferrocene Moles of limiting reagent 1.21*10^-3 mol Final weight of product 0.288g Theoretical yield 29.49 Moles of product 3.73*10^-4 mol % yield 97% melting point (°C) of product 128°C -131°C Calculations: Moles of Ferrocene 0.225g * mol of ferrocene/186
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(important details) How can the rxn be activated Second step: rxn of the Grignard reagent with acetophenone‚ quenching with ammonium chloride Isolation of the product‚ identification Possible or actual sources of error Part one of our experiment consisted of the preparation of phenylmagnesium bromide from bromobenzene. PhMgBr is an organometallic reagent‚ a class of nucleophile known as a Grignard reagent. Gringard reagents are a class of extremely reactive chemical compounds used in the synthesis of
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Title: Finding the Ratio of Mole of Reactants in a Chemical Reaction Purpose of Lab: To find the coefficients of two chemical reactants that appears in a balanced chemical equation using the continuous variations method. Pre Lab Questions: 1. 2AgNO3(aq) + K2CrO4(aq) → 2KNO3(aq) + Ag2CrO4(s) 2. There is enough to make a valid conclusion because‚ on the graph‚ one can clearly see that the two lines intersect. Thus‚ one can also determine the mole ratio. The mole ratio is approximately
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interest. If it is desired to measure either organic or inorganic COD alone‚ additional steps not described here must be taken to distinguish one from the other. COD is a defined test; the extent of sample oxidation can be affected by digestion time‚ reagent strength‚ and sample COD concentration. COD often is used as a measurement of pollutants in wastewater and natural waters. Other related analytical values are biochemical oxygen demand (BOD)‚ total organic carbon (TOC)‚ and total oxygen demand (TOD)
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crystal was weighed. The melting point range of the recrystallized tin tetraiodide was measured using a MEL-TEMP. Instruments should be washed by acetone during the experimental. Result Table 1 contains the molar mass‚ mass and the moles of reagents (Sn and I2) and products (crude SnI4‚ recrystallized SnI4 and air-dry SnI4). The yields of product and percent recover of
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three-membered ring intermediate. 3. Below is the reaction equation for the experiment and shows the possible identities for the product. II. Key experimental details‚ observations‚ and results: Table 1: Exactly how much of each reagent was used Reagent | Amount added to flask | (E)-stilbene | .201g | Glacial Acetic Acid | 4.1mL | Pyridinium Tribromide | .391g | A. Observations: 1. The 10mL round-bottom flask weighed 17.690g. 2. The flask was heated and stirred at ~95
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veterinarian clinics. Omnivue is one of the most successful equipments produced by the company‚ which is priced at a competitive rate to attract lower and middle sized veterinarians. The production of Omnivue involves the use of plastics and chemical reagents supplied by two major suppliers‚ GenieTech and Elsinore. The management of Bergerac is planning to take control over its suppliers to reduce the production fluctuation and overhead costs of the firm. There are three strategic alternatives for the
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submitted: 05/09/05 Chem 2130-3 Experiment 3: Synthesis of Co(acac-NO2)3 Introduction In this lab‚ Co(acac·NO2)3 is synthesized using the Co(acac)3 complex produced in Experiment 2. The Co(acac)3 complex is used as a reagent instead of acacH because acacH cannot be directly converted to 3-nitroacetylacetone. Since Co(acac)3 is not stable in HNO3‚ Cu(NO3)2 and acetic anhydride are used in this reaction to produce the final product‚ Co(acac·NO2)3. The exact mechanism
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beaker with the HCl and record the mass. 5. Carefully add the marble chips and gently stir until all the CaCO3 is dissolved 6. Weigh the beaker again and record the mass. VI. Results and Calculations 7. Find the limiting reagent 8. Find the theoretical yield by multiplying the amount of moles of the limiting reactant to the molar ration of limiting reactant : ratio and by the molecular weight of the product. 9. Find the percentage yield --> Pecentage
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g KClO3 X ( 1 mol / 122.55 g ) = 1.131 mol KClO3 3. Determine the limiting reagent [if necessary] (Use mole ratios to figure out.) * Not necessary to determine because there is only 1 reactant in this decomposition reaction. 4. Use ratios to find the moles of the reactant or product you need to find. Since KClO3 is the only reactant‚ it is the limiting reagent. You use the moles of KClO3 if you have to calculate how many moles of oxygen gas (the
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