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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The Equilibrium Constant of an Ester Hydrolysis Reaction Julia Stanley CHM 152 LL Dr. Asmita Kane Budruk Goal of the lab: The purpose of this laboratory is to determine the equilibrium constant‚ Kc‚ for the acid-catalyzed reaction between an unknown ester and water to produce an unknown alcohol and an unknown carboxylic acid. I was using Unknown Ester #3 with a density of 0.9342 and Molar Mass of 74.08 g/mol; alcohol with density 0.7914 and Molar Mass 32.04 g/mol. Chemical
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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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simply cross-check your homework questions with this Question Bank and wrap up your homework in record time! Chemistry Some Basic Concepts of Chemistry Mass and Stoichiometry Chemistry > Chapter: Some Basic Concepts of Chemistry > Mass and Stoichiometry Chapter: Some Basic Concepts of Chemistry Mass and Stoichiometry Question 1 2.5 moles of sulphuryl chloride were dissolved in water to produce sulphuric acid and hydrochloric acid. How many moles of KOH will be required to completely
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Stoichiometry • Calculations involving quantities of consumed reactants and formed products based on a BALANCED chemical equation. Mass Molar Mass Mole Coeff Bal Eqn Mole Molar Mass Mass Example 2 • The Haber Process involves reacting gaseous nitrogen and gaseous hydrogen to form ammonia. Determine the mass in grams of hydrogen gas required to form 1.00 x 103 g ammonia. Your Turn 2 • If you react 52.9 g of potassium chlorate (KClO3) with excess phosphorus
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Experiment 4 SOLUTION STOICHIOMETRY ACID-BASE TITRATIONS Determination of the Percent Acetic Acid in Vinegar Objectives: (1) To introduce and use the concept of solution stoichiometry (2) To specifically use solution stoichiometry to determine the percent of acetic acid in vinegar. (3) To prepare a standard solution by the method of titration. Consider the following balanced chemical equations: (1) HCl + NaOH ------> NaCl + HOH (2) H2SO4
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to describe the reactions and observations from the laboratory activity. Lesson 4.06: Stoichiometry Explain what the coefficients in a balanced equation represent and how they can be used in ratios. Use coefficients from a balanced equation as a mole ratio in dimensional analysis calculations. Solve a variety of stoichiometry calculations involving moles and mass. Use volume and density in stoichiometry calculations (honors). Lesson 4.07: Limiting Reactant Identify when a problem
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Exam Review Sheet #1 Balancing Equations and Simple Stoichiometry Answers are provided on the second sheet. Please try to do the worksheet without referring to them‚ because you’ll be expected to know this stuff the first day of school! Balance the following equations: 1) ___ N2 + ___ F2 ( ___ NF3 2) ___ C6H10 + ___ O2 ( ___ CO2 + ___ H2O 3) ___ HBr + ___ KHCO3 ( ___ H2O + ___ KBr + ___ CO2 4) ___ GaBr3 + ___ Na2SO3 ( ___ Ga2(SO3)3 + ___ NaBr 5) ___ SnO + ___ NF3 ( ___ SnF2
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Problem Set Introduction to Stoichiometry Name: ______________________________________________________ Course/Yr/Section: ____________ Date:_____________ Direction: Analyze and solve each problem carefully‚ write the solution on the space provided. Box your final answer/s. (10pts each) Determine the molar mass of the following: a. Al(NO3)3 b. ZnSO4 c. Ba(C2H3O2)2 d. NaHCO3 CH3COOH Calculate the percentage oxygen in the following compounds: a. Na2CO3 b. BaSO4 c. BaO
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Amanda Tran Date of lab: 04/25/05 Date 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
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