mixing the two reactants with NaOH and ethanol‚ then allowing the reaction to sit for thirty minutes. The crystals were then washed with water three times and recrystallized using ethanol. It was then characterized using melting point analysis. The percent yield for this reaction was 59.84%. This was due to loss of crystals during recrystallization and during solvent removal from the reaction mixture. The observed melting point was 104 – 107.5°C‚ compared to a literature value of 110°C. The lower and broader
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carboxylic acid (acetic acid)‚ adding three drops of sulphuric acid acting as a catalyst to produce an ester (isopentyl acetate) and water. We verified our answers using infrared spectroscopy. Calculations for Percent Yield To find the percent yield we had to first find moles of our limiting reagent. 1) Weight of 5mL vial + cap
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calculations: Mass of product‚ Limiting reagent‚ Theoretical yield‚ Percent yield‚ melting point of product. State integration‚ chemical shifts of all peaks or reagions of peaks and Splitting (singlet‚ triplet‚ quartet). If there are many peaks jumbled in one area such as in the aromatic region‚ state the beginning and ending chemical shift‚ the integration‚ and call the peak a “multiplet” Use the areas of the methylene peaks at 4.7 and 3.9 ppm to determine the percent composition of each product
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in a precipitation reaction. We received working knowledge of how to accurately measure reactants and products of the reaction. We then are able to use the data that we recorded to make assessments of the actual yield opposed to the theoretical yield. When we calculated the percent yield we are able to see how accurate the data we recorded is. Experiment and Observation: The first thing we needed to do for this experiment was to weigh 1.0 g of CaClᴤ ˣ 2HᴤO and placed it into a 100 mL beaker
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reactants (usually the cheaper one). • Limiting Reactant – reactant that will be totally consumed. • Excess Reactant – will not be totally consumed; will have left over. • The maximum amount of product (theoretical yield) that can be obtained in a chemical reaction is based on the limiting reactant. – Need to fully “GRASP” Example 3 • Consider the reaction: 2Sb (s) + 3I2 (s) → 2SbI3 (s) Determine the limiting reactant and the theoretical yield (in grams) when 1.20 g of Sb and 2.40
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characterized by the combining of an alcohol and an acid (with an acid catalyst) to yield and ester plus water. In order to accomplish this reaction‚ the reactants were refluxed for 30 minutes at 80 degrees Celsius ‚to yield a mixture‚ the mixture was then mixed with sodium hydrogen carbonate and dried with anhydrous sodium sulfate. The product obtained from this reaction was then weighed and yielded 3.5753g‚ the total percent yield of isopentyl acetate obtained was 60 %. The advantages of using this particular
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Abstract: The objective of this lab is to calculate the theoretical‚ actual‚ and percent yield of the product from a precipitation reaction. It is also to learn concepts of solubility and the formation of a precipitate. The Experiment and Observation: Weigh out your 1.0g of CaCl2-2H20 and put it into the 100mL beaker‚ add your 25mL of distilled water and stir to form the calcium chloride solution. Next‚ use stoichiometry to determine how much Na2CO3 and put it into a small paper cup. Then add
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acid as a catalyst. The product was washed with sodium hydrogen carbonate‚ as well as with water‚ then dried with anhydrous sodium sulfate. The product was then distilled using a Hickman still and characterized using infrared spectroscopy. The percent yield of isopentyl acetate was 61.52%. This may have been low due to not all of the condensed product being removed from the Hickman still‚ some product being lost during transfer of the product from the reaction tube into the Hickman still‚ or the loss
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A solution of cyclohexene‚ aqueous sodium hydroxide‚ and benzyltriethylammonium was used to synthesize 7‚7 – dichloronorcarane by the following reaction: + CHCl3 + OH - H2O + + Cl - After completion of the experiment‚ the percent recovery was calculated to be 46.21% Introduction The purpose of this experiment was to form 7‚7-dichloronorcarane by means of carbene trapping. Cyclohexene‚ aqueous sodium hydroxide‚ and benzyltriethylammonium chloride were used to synthesize
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hydrogen gas collected. pv=mrt ; n= .0013mol of hydrogen gas 4. If magnesium was the limiting reactant in this lab‚ calculate the theoretical yield of the gaseous product. Show all steps of your calculation. 0.03184 g Mg(1mol Mg/ 24.3050 g Mg)= 0.0013mols Mg 0.0013mols Mg(1mol H2/ 1mol Mg)= .0013 1. Determine the percent yield of this reaction‚ showing all steps of your calculation. 2. (actual yield/ theoretical yield)x 100% (0.0013/ 0.0013)x 100= 100% 1. Would the following errors increase‚ decrease
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