silver nitrate to react with the salt from perspiration produced 5.8 x 10-2 grams of silver chloride. How many grams of salt was left by the initial latent fingerprint? Brainstorm the steps to solve this problem as you recall the steps to solving stoichiometry calculations. Be prepared to explain your solution including your decisions with significant figures and scientific notation to increase accuracy. Be sure you complete each step of the process: 1. Write the chemical equation. AgNO3 + NaCl
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Mass (g/mol) Amount used (moles) Melting point (Celsius) Color/observations 2‚3-dibromo-3-phenylpropanoic acid 0.285g 307.97 200.4 – 205.1 White powder Limiting reagent: Trans-cinnamic acid (148.16g/mol) 2.5g/148.16g/mol=0.01687mol Stoichiometry ratio: 1:1 ratio Theoretical yield: Since 0.01687 moles of trans-cinnamic acid therefore following the 1:1 ratio one concludes that 2‚3-dibromo-3-phenylpropanoic acid will be of 0.01687 moles Molar mass = 307.97 g/mol Mass=(307.97g/mol)(0.01687mol)=5
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aliquots of sample solution until you obtain concordant results (titres agreeing within 0.1 mL). 37. Record findings 38. Subtract the initial volume to determine the amount of titrant delivered. Use this‚ the concentration of the titrant‚ and the stoichiometry of the titration reaction to calculate the number of moles of reactant in your analyte solution. 39. Then Calculate the results 40. 1. Calculate the average volume of iodate solution used from your concordant titres. 41. 2. Calculate the moles
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DEPARTMENT OF PURE AND APPLIED CHEMISTRY Visayas State University Visca‚ Baybay City‚ Leyte Name: Alecsa May S. Celaya BS-Chemistry 3 Date Submitted: December 19‚ 2014 Lab. Schedule: MW 2:00 – 5:00 pm Rating: Group No. 11 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
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| Percent Yield Lab | | | | 4/20/2012 | Mrs.Sardella Per4 Matt ‚ Kait Mrs.Sardella Per4 Matt ‚ Kait | Introduction *Limiting Reactant: A reactant that is completely consumed during a chemical reaction‚ limiting the amount of product that is produced. *Excess Reactant: A reactant that remains after a reaction is over. *Theoretical Yield: The amount of product that is predicted by stoichiometric calculations *Actual Yield: The amount of product that is recovered
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CHEMISTRY Safety‚ Matter‚ and Measurement Lab Safety Dress appropriately Follow directions and act appropriately Know where emergency equipment is MSDS Material Safety Data Sheets- contain safety information about chemicals Converting metric units Kilo Hecto Deca Base Deci Centi Milli 1000 100 10 1 1/10 1/100 1/1000 Significant Figures NOT Significant Digits “Placeholders”- Zeros before the decimal point and after the number
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equilibrium constant‚ Kc‚ that relates the concentrations of all product and reactant species‚ (2) where [A]‚ [B]‚ [C]‚ and [D] are the molar concentration of all species present at equilibrium. The exponents‚ a‚ b‚ c‚ and d represent the stoichiometry coefficients from the balance chemical reaction. Kc is really the ratio of the rate of the reverse reaction divided by the rate of the forward reaction and so is a dimensionless constant at a given temperature. Additionally‚ functional groups
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Chem 201 Lab October 21‚ 2011 Lab #6: Preparation of 2-chloro-2-methylbutane – an Sn 1 Reaction Purpose The purpose of this experiment was to prepare an alkyl halide‚ 2-chloro-2-methylbutane by reacting 2-methyl -2-butanol (t-amyl alcohol) with hydrochloric acid. Alkyl halides are of wide interest because they are widespread and have diverse beneficial and detrimental impacts .The overall reaction is given below: Procedure 1 ml of 2-methyl-2-butanol was measured using 1 ml syringe and
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percent yields will be determined and reported. Objective: To determine the limiting reactant‚ theoretical yield‚ actual yield‚ and percent yield in a chemical reaction between solutions of potassium iodide and lead (II) nitrate. Introduction: Stoichiometry‚ mass‚ and mole relationships have been important throughout the history of chemistry. The simplest whole number relationship between the products and the reactants is a chemical equation. If the masses or number of moles of reactants are known
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combining the elements‚ instead of having it naturally do so‚ made a significantly fully more bright color. In Theophilus’s “recipe” for vermillion‚ it is stated that there should be far more sulfur than a stiochiometric reaction should require. Stoichiometry
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