com/mdc/public/page/2_3020-treasury.html?mod=topnav_2_3000 and find out the ask/bid price quotes and asked yields for treasury bills (1) maturing on 2009/09/24‚ traded on 2008/09/24 Bid = 1.845 Ask = 1.835 Asked yield = 1.887 (2) maturing on 2010/09/23‚ traded on 2009/09/24 Bid = 0.385 Ask = 0.378 Asked yield = 0.384 (3) maturing on 2011/09/22‚ traded on 2010/09/24 Bid = .250 Ask = .245 Asked yield = .249 2. Calculate the ask prices for the above three T-bills using bank discount method. (1)
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involving filtration‚ sedimentation‚ decantation and extraction. While different reaction were also observe and tallied until the recovered copper was weight and the percentage yield was calculated from the formula: Percentage Yield = Mass of recovered copper/ actual yield mass of copper wire(Theoretical yield) X 100 The Percentage Yield of the experiment was 87.63% INTRODUCTION All chemicals reactions occurring within test tube‚ industrial reactors‚ or nature‚ can be described by reaction equations
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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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The purpose of this experiment is to use stoichiometry to predict how much of a product will be made in a precipitation reaction‚ to measure the reactants and products of the reaction correctly‚ to figure out the actual yield vs. the theoretical yield and to calculate the percent yield. Procedure First‚ 1.0 g of CaCl2·2H2O was put into a 100-mL beaker and 25 mL of distilled water was added. The two ingredients were stirred to create a calcium chloride solution. Then‚ stoichiometry was used to
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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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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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is trading for a price of $1034.74. a. What is the bond’s yield to maturity (expressed as an APR with semiannual compounding)? b. If the bond’s yield to maturity changes to 9% APR‚ what will the bond’s price be? 6-10. Suppose a seven-year‚ $1000 bond with an 8% coupon rate and semiannual coupons is trading with a yield to maturity of 6.75%. a. Is this bond currently trading at a discount‚ at par‚ or at a premium? Explain. b. If the yield to maturity of the bond rises to 7% (APR with semiannual compounding)
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account. The percent yields for the reactants in the equation are very far from 100% yield. In the case of water‚ the percent yield came out to be meaning there were at least 2 times to 4 times more water than there should be. The percent yield of oxygen came out to be ‚ around 2%‚ maybe higher considering uncertainty of what amount of oxygen there was suppose to be. The reaction was incomplete and had to be stopped because of time‚ which explains the very high percent yield of the water and the
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Organic Chemistry I – CHEM 201-DL01 September 26‚ 2014 Organic Chemistry Experiment 4B Lab Report Extraction of Organic Compounds From Natural Sources: Extraction of Trimyristin From Nutmeg Introduction The purpose of this experiment is to illustrate how a solid natural product can be extracted from its natural source through the use of an organic solvent. Natural products are organic compounds that are synthesized by natural biological processes in plants‚ animals
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Abstract: This experiment involved a reaction between anthracene and maleic anhydride via a Diels Alder reaction to yield 9‚ 10-dihydroanthracene-9‚10-α‚ β-succinic anhydride. Anthracene was the diene and maleic anhydride was the dienophile. The percent yield of the crude product was 69.03%. Following recrystallization of the product using xylene and vacuum filtration‚ a percent yield of 37.42% for the recrystallized product was collected. This was low due to the fact that some of the crude product
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