Ethyl Acetate – NaOH Reaction Kinetics Experiment Martin Novick Group 14‚ Chemical Engineering Laboratory Submitted to Prof. David B. Henthorn September 25‚ 2012 Summary The goal of this project was to determine the pre-exponential factor‚ k o ‚ the activation energy‚ E‚ and the reaction rate constants‚ k‚ of the saponification process of ethyl acetate using sodium hydroxide (NaOH) at 5 temperature between 15 and 25 degrees Celsius. Two trails were performed at temperatures 16‚ 18‚ 20‚ 22‚ and 24
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Determining the Enthalpy of a Chemical Reaction All chemical reactions involve an exchange of heat energy; therefore‚ it is tempting to plan to follow a reaction by measuring the enthalpy change (∆H). However‚ it is often not possible to directly measure the heat energy change of the reactants and products (the system). We can measure the heat change that occurs in the surroundings by monitoring temperature changes. If we conduct a reaction between two substances in aqueous solution‚ then the
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Experiment I: Thermochemistry Background: Thermochemistry is the branch of chemistry that focuses on the studies of chemical reactions or physical changes and heat associated with chemical reactions. According to the first law of thermodynamics‚ energy cannot be created or destroyed but it can be converted from one form into another and/or transferred between different atoms‚ molecules‚ or substances. In general‚ energy can be classified into two categories: kinetic and potential. Kinetic energy
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(C) NH2– (D) H3O+ (E) NaOH 3. In this reaction‚ CH3COOH + H2O H3O+ + CH3COO–‚ which substances are bases according to the Brønsted–Lowry definition? (A) CH3COOH and H2O (B) CH3COOH and CH3COO- (C) H2O and CH3COO– (D) H3O+ and CH3COO– 4. In the reaction CN– + H2O HCN + OH–‚ which is an acid–base conjugate pair? (A) H2O and HCN (C) CN– and H2O (B) H2O and OH– (D) HCN and OH– 5. Which species is not either an Arrhenius acid or base? (A) HCO3– (B) NaOH (C) HIO4 (D) NH3 6. When
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06.03 Calorimetry: Lab Report Before You Begin: You may either copy and paste this document into a word processing program of your choice or print this page. Procedure: Part I: The Dissolving of Solid Sodium Hydroxide in Water Measure out approximately 205 mL of distilled water and pour it into the calorimeter. Stir carefully with a thermometer until a constant temperature is reached. Record the volume of water and the constant initial temperature of the water on your data table. Place
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Title : Expt.1 Determination of the enthalpy (heat) of reaction of a monobasic acid with sodium hydroxide Experiment no : 1 Experiment title : Determination of the enthalpy (heat) of reaction of a monobasic acid with sodium hydroxide Objectives: 1) To understand the enthalpy chemistry. 2) To determine the calorimeter constant. 3) To determine the enthalpy reaction of acid-base reactions. 4) To study the exothermic reaction. Apparatus and Materials : * Dewar flask
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In part A‚ solutions needed in the experiment were prepared‚ and the LabQuest was set up. By adding 100mL 6M HCl to 200mL deionized water‚ 300mL of 2M HCl solution was prepared. Then 150mL 2M NaOH solution was prepared by adding 100mL 3M NaOH to 50mL deionized water. Finally‚ the LabQuest was connected to the temperature probe‚ and set up to collect data every 15 seconds‚ the duration was set to be 180 seconds. In part B‚ three reactions were performed. In reaction 1‚ two Styrofoam cups were stacked
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that can be added is equal to the amount of conjugate base present in the buffer. The maximum amount of base that can be added is equal to the amount of weak acid present in the buffer. DATA Concentration of Buffer Trial 1 Trial 2 0.1 M ml NaOH pH 0 4.57 0 4.64 0.5 4.75 0.1 4.66 1.2 4.95 0.5 4.74 2.4 5.28 0.7 4.8 3 5.56 1 4.85 3.3 5.75 1.5 5 1.8 5.06 2 5.1 2.2 5.18 2.5 5.28 2.8 5.4 3.1 5.6 3.5 5.93 0.3 M 0 4.75 0 4.89 0.4 4.78 1.8 4.96
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the mass. (The weight of the weigh boat was zeroed out prior to measuring the salt). Once we added the salt to the ammonia and completely mixed the solution‚ we pipetted 20 mL into a volumetric flask. Then we set up a titration system using 0.100M NaOH in the buret. For the step-by-step procedure guidelines‚ refer to‚ “Investigations of Buffers. CHM 116 Spring 2013 Lab Manual‚ Grand Valley State University pages 49-56” III. Data Ammonia/Ammonium Buffer. Table I. Titration
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1. Clean‚ rinse‚ and fill a buret with NaOH solution just as you did in last week’s experiment. Record the molarity of the NaOH and the initial NaOH volume reading from the buret (+0.02 mL). 2. Weigh an antacid table in a weighing boat and record the mass (+0.01 g). Transfer the tablet to a clean mortar and crush the tablet into a fine powder using the pestle. 3. Weigh about 0.2 grams (+0.01 g) of the ground up tablet powder and transfer it to a clean 250 mL Erlenmeyer flask. 4. Transfer
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