__________________________________________________ Purposes: 1. Calculate theoretical mass of NaCl based on a known mass of NaHCO3. 2. Experimentally determine the actual mass of NaCl produced. 3. Calculate the percent yield for your experiment. Reaction Equation: NaHCO3(s) + HCl(aq) ( NaCl(s) + CO2(g) + H2O(l) Materials: safety glasses baking soda (NaHCO3) 1 M HCl and dropper 500 ml Pyrex flask hot plate Procedure: 1. Find
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Mass of filter paper and dry calcium carbonate __1.8__g Net mass of the dry calcium carbonate __.8__g (This is the actual yield) Step 11: Show the calculation of the theoretical yield of calcium carbonate. .0068 mol of CaCO3 *100.06 g CaCO3/1mol of CaCO3 =.6804 g of CaCO3 Show the calculation of the percent yield. (Actual yield/theoretical yield)*100 = (.8/.68)*100 =117% Conclusion: The primary objectives of this experiment were to predict the amount of
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Preparation of Bromotriphenylmethane Abstract The structure of a major component of star anise oil was derived by analyzing its IR spectroscopy melting point of after oxidation and purification. From the evidence obtained‚ it was concluded that the exact structured should be p-methoxybenzoic acid. Introduction The purpose of this experiment is to determine the structure of the major component of star anise oil. It is already known that this component has a molecular formula C10H12O. This
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Experiment No. 5 Preparation of KAl(SO4)2•12H2O (Alum) OBJECTIVES This experiment aimed to: prepare KAl(SO4)2•12H2O‚ commonly referred to as alum‚ from aluminum metal from a canned soft drink‚ and determine the mass of the alum collected and its percent yield. METHODOLOGY An aluminum metal scrap was obtained by scraping the paint off a Coca-Cola can. It was then cut into small pieces and was placed in a pre-weighed 250 mL beaker. With the use of an analytical balance‚ by taring the mass of the beaker
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CaCO3 theoretical yield as follows: 1 g CaCl2·2H2O x 1 mole CaCl2·2H2O x 1 mol CaC03 x 100 g CaC03 = 147 g CaCl2·2H2O 1 mol CaCl2·2H2O 1 mol CaC03 To double-check‚ we can calculate CaCO3 theoretical yield by using Na2CO3 0.72 g Na2C03 x 1 mol Na2C03 x 1 mol CaC03 x 100 g CaC03 = 106 g Na2C03 1 mol Na2C03 1 mol CaC03 www.LabPaq.com 56 ©Hands-On Labs‚ Inc. Experiment Stoichiometry of a Precipitation Reaction Questions A. From your balanced equation what is the theoretical yield of your product
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Name: David Kennedy Date: 11/5/14 Project No: 131 Title: Butyl 2-Cyano-(3‚5 dichloro-phenyl)-2-propenoate Abstract: The targeted trisubstituted ethylene compound Butyl 2-Cyano-(3‚5 dichloro-phenyl)-2-propenoate and its copolymer with styrene was prepared in this lab. The base catalyzed Knoevengael condensation of butyl cyanoacetate and corresponding aldehyde led to the forming Butyl 2-Cyano-(3‚5 dichloro-phenyl)-2-propenoate. The analyses that were used to prove its composition and structure
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Abstract A Friedel-Crafts alkylation was performed by adding t-butyl alcohol to p-dimethoxybenzene in order to produce 1‚4-di-t-butyl-2‚5-dimethoxybenzene. This reaction yielded 0.009g of 1‚4-di-t-butyl-2‚5-dimethoxybenzene having a percent yield of 5%‚ and a melting point range of 54.8°C-56.9°C. Introduction This reaction is designed to put functional groups onto aromatic rings. This is done through an electrophilic aromatic substitution where a positive species is strong enough to pull electrons
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1.PERCENT ● DEFINITION OF PERCENT - Percent means parts per 100 The symbol is % Example: 25% means 25 per 100 ● CONVERSION TECHNIQUES - ✔Changing percent to decimal Change a percent to a decimal. Move the decimal point two places to the left. In a percent‚ the decimal point would come at the end of the last number (for 75%‚ envision that it looks like 75.) Examples: 75% converts to .75 40% converts to .40 3.1% converts to .031 ✔Changing decimal or whole number to percent Change a decimal
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the most important. Include observations such as appearance of the reaction‚ color of product‚ etc. If the experiment was a preparative one‚ you should also report your percent yield: Percent Yield = Actual or experimental yield in grams (or moles) X 100 Theoretical or calculated yield in grams (or moles) Show all of your calculations! Graphs should be done on graph paper. Note: Our lab manual contains a "Data Report Sheet" for each experiment
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Nitration of Naphthalene Wed 2/25/2015 Lab report # 1 Abstract: The purpose of this experiment was to nitrate naphthalene with nitronium ion‚ which is formed at low concentration from a reaction of nitric acid and sulfuric acid. The percent yield from the experiment was 54.4% of the product‚ and the melting point of the possible results were 59 °C for 1-nitronaphthalene‚ and 78°C for 2-nitronaphthalene. Introduction: Polynuclear aromatic hydrocarbons such as naphthalene can be nitrated
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