Green Chemistry: As American as Apple Pie. Synthesis of Banana Oil Using Green Chemistry. AAS in Chemical Technology. Background
|
|
- Morgan Horton
- 6 years ago
- Views:
Transcription
1 Synthesis of Banana il Using Green hemistry Pamela Brown Simon Dexter New York ity ollege of Technology Brooklyn, NY Green hemistry: As American as Apple Pie As educators we have the opportunity to influence future generations of chemists The laboratory presented today was developed with an undergraduate, Simon Dexter, as an honors project in General hemistry II. AAS in hemical Technology Background General hemistry I and II (8 credits) rganic hemicstry I and II (1 credits) Analytical hemistry I and II ( 9 credits) Introduction to Physical hemistry (3 credits) Science Research Skills (3 credits) Physics I and II ( 8 credits) Pre-alculus ( 4 credits) English I and II ( 6 credits) Psychology (3 credits) Liberal Arts Electives ( 6 credits) Synthesis of esters, especially 3- methylbutylacetate, banana oil, is a classic experiment performed in organic chemistry labs across the country. Traditionally, the Fisher esterification is performed: H 2 H H 2 H H = H H 2 H 2 H 2 isopentanol acid isopentyl acetate water 3-methylbutanol acetic acid= 3-methylbutylacetatewater Eq. 1
2 Background The reaction uses sulfuric acid as catalyst and requires about one hour of reflux to reach equilibrium where: Keq = 4.2 At equilibrium the yield is only about 67%. An ether, such as ethyl ether is added to extract the banana oil. The banana oil is recovered by fractional distillation. Microwave Induced Heating Microwave radiation rapidly heats polar substances. Polar substances try to align themselves with the electric field. Since the frequency is 245 MHz the molecules don t have time to line up one way before they have to line up the other way. The resulting friction causes the solution to heat up. 3-Methylbutylacetate Synthesis with Microwave Heating Stoichiometric amounts of acetic anhydride (7. ml=.74 moles) and 3-methylbutanol (8. ml =.74 moles) are mixed in an HP5 pressure vessel and heated in a EM MARS Microwave oven with temperature control at ambient pressure for 8 minutes at 11, after a 2 minute ramp to the reaction temperature. 3-methylbutylacetate acetic anhydride= 3-methylbutylacetate acetic acid H H 2 H H 2 H == H H 2 H Determination of Yield The products are titrated using 2. M NaH. The sample separates into 2 phases, an organic phase containing essentially pure 3-methylbutylacetate (average yield = 9%), and an aqueous phase containing sodium acetate. Titration results can be used to calculate the yield. Acetic Anhydride water! 2 Acetic acid Acetic Acid NaH! Sodium acetate water Moles 3-methylbutylacetate produced = 2X initial moles of acetic anhydride - moles of acetic acid in product = 2X initial moles of acetic anhydride - moles of NaH to titrate product
3 Why is this an example of green chemistry? Eliminates the need for using sulfuric acid as a catalyst, and ether for the extraction Eliminates the need for fractional distillation Reduces energy consumption Additional Applications Last summer an undergraduate, Alyse Rich, supported by an NIH Bridges grant and a high school student, Vincent ng, supported by an AS SEED grant studied the rates of reaction using microwave heating and compared them to conventional heating. Reactions Studied 3-methylbutanol acetic anhydride _ 3-methylbutylacetate acetic acid H H 2 H H 2 H == H H 2 H ethanol acetic anhydride _ ethylacetate acetic acid H H == 3 H 2 H 2 H Determination of Rate Equation A! B First rder Reaction:-d[A]/dt = k[a] Plot of ln[a] vs t is a straight line, slope = -k Second rder Reaction d[a]/dt = k[a] 2 Plot of 1/[A] vs t is a straight line, slope = k
4 Procedure Two equimolar samples of acetic anhydride and alcohol were prepared (~15 ml total volume) ne was heated for a given time and temperature (T=8, 9, 11 with 3-methylbutanol and T=7, 75, 82 with ethanol) in a EM Microwave reactor with temperature control. The second was heated in a constant temperature oil bath. The % of unreacted acid = RH and the % yield of ester was determined by titration. Plots of % RH vs time, ln (% RH) vs time and % RH -1 vs time were prepared to determine the reaction order, rate constant and activation energy Plot of 1/ % RH vs Time at 8 for microwave heating slope = k Figure 1- Banana oil synthesis- Microwave Heating min ramp to 8 = time ml 2M NaH time (min) % Yield time (min) 1/(% reactant) /% reactant % Yield /%reactant vs time(min)-8 microwave time (min) % Yield vs Time - Microwave Heating - 8 y =.16x.99 R 2 = Time (minutes) Arrhenius Equation: k = A exp (-E/RT) Plot of ln k vs 1/T for microwave heating- slope = -E/R Figure 5 - ln k vs 1/T(K) - banana oil synthesis - microwave heating k Temperature() 1/T(K) ln(k) Experimental Activation Energies Reaction E a, Activation Energy (kj/mole) A, Arrhenius onstant ln k Determination of Activation Energy and Arrhenius onstant- Ln k vs 1/T(K) /T(K) y = x R 2 =.9659 Ethylacetate synthesis conventional heating x 1 24 Ethylacetate synthesis microwave heating x 1 13 Banana oil synthesis microwave heating and conventional heating x 1 7
5 Discussion With ethanol, the rate of reaction was 2-3 times greater with microwave heating than conventional heating. With 3-methylbutanol the rates were equal. This suggests that the alignment of molecules due to the oscillating electric field produced by the microwaves may have a catalytic effect on smaller alcohols. onclusion Introducing Green hemistry Labs into the curriculum reduces waste generated by the college and creates a culture of respect for the environment Encouraging students to develop these labs is an opportunity to develop short-term student projects with tangible results
Chemical Kinetics Ch t ap 1 er
Chemical Kinetics Chapter 13 1 Chemical Kinetics Thermodynamics does a reaction take place? Kinetics how fast does a reaction proceed? Reaction rate is the change in the concentration of a reactant or
More informationR C OR' H 2 O carboxylic acid alcohol ester water side product
EXPERIMENT 7 SYNTHESIS OF ESTERS USING ACETIC ANHYDRIDE 1 Materials Needed 2.0 ml of an alcohol to be chosen from the following: 1-propanol (n-propyl alcohol), 3-methyl 1-butanol (isoamyl alcohol, isopentyl
More informationORGANIC SYNTHESIS: MICROWAVE-ASSISTED FISCHER ESTERIFICATION
EXPERIMENT 7 ORGANIC SYNTHESIS: MICROWAVE-ASSISTED FISCHER ESTERIFICATION Materials Needed 1.0-2.0 ml of an alcohol to be chosen from the following: 3-methyl 1-butanol (isoamyl alcohol, isopentyl alcohol),
More informationCHEM 254 EXP 10 Chemical Equilibrium - Homogeneous and Heterogeneous Equilibrium
Gibbs energy, G CHEM 254 EXP 10 Chemical Equilibrium Homogeneous and Heterogeneous Equilibrium A reaction at constant temperature and pressure can be expressed in terms of the reaction Gibbs energy. The
More informationCHEMICAL ENGINEERING LABORATORY CHEG 4137W/4139W. Reaction Kinetics Saponification of Isopropyl Acetate with Sodium Hydroxide
CHEMICAL ENGINEERING LABORATORY CHEG 4137W/4139W Reaction Kinetics Saponification of Isopropyl Acetate with Sodium Hydroxide Objective: The purpose of this experiment is to examine and determine the reaction
More informationChemical Kinetics. Chapter 13. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Chemical Kinetics Chapter 13 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chemical Kinetics Thermodynamics does a reaction take place? Kinetics how fast does
More informationln(k) = ( E a /R) (1/T) + ln(a) Copyright 2018 Dan Dill 1
TP For A B, is 0.003/min at 25 o C and 0.025/min at 35. For C D, is 0.003/min at 25 and 0.035/min at 35. Compared to the activation energy of A B, the activation energy of C D is 1. smaller 2. the same
More information13. Chemical Equilibria
13. Chemical Equilibria Many reactions are reversible + 3 2 All reversible reactions reach an dynamic equilibrium state. Dynamic equilibrium occurs when forward and backward reactions are occurring at
More informationb. The water is more attracted to the unreacted alcohol and acid than to the ester.
End of Lab Questions 1/30/18 Lab 1, Part C, Day 2 1. a. What lab technique did you use to separate the ester from the impurities? Liquid-liquid extraction b. The water is more attracted to the unreacted
More informationAll reversible reactions reach an dynamic equilibrium state. H 2 O+ CO H 2 +CO 2. Rate of reverse reaction (H 2 + CO 2 )
4.2 Equilibria Many reactions are reversible + 3H 2 2NH 3 All reversible reactions reach an dynamic equilibrium state. Dynamic equilibrium occurs when forward and backward reactions are occurring at equal
More informationAll reversible reactions reach an dynamic equilibrium state.
11. Equilibrium II Many reactions are reversible + 3 2NH 3 All reversible reactions reach an dynamic equilibrium state. Dynamic equilibrium occurs when forward and backward reactions are occurring at equal
More information1.6 Equilibria All reversible reactions reach an dynamic equilibrium state.
1.6 Equilibria All reversible reactions reach an dynamic equilibrium state. Many reactions are reversible + 3 2NH 3 The term dynamic means both forward and backward reactions are occurring simultaneously
More informationCHEM 1412 Practice Exam 1 - Chapters Zumdahl
CHEM 1412 Practice Exam 1 - Chapters 11 13 Zumdahl Some equations and constants: T = Km P = XP = MRT ln[a]t = kt + ln[a]o 1 / [A]t = kt + 1 / [A]o t1/2 = ln(2) / k t1/2 = 1 / k{a]o Kp = Kc(RT) n ln(k1/k2)
More information5.1.2 How Far? Equilibrium
5.1.2 How Far? Equilibrium Equilibrium constant Kc Kc = equilibrium constant For a generalised reaction ma + nb pc + qd [ C] p [D] q m,n,p,q are the stoichiometric balancing [ A] m [B] n numbers A,B,C,D
More informationWINTER-15 EXAMINATION Model Answer
Subject code :(735) Page of 9 Important Instructions to examiners: ) The answers should be examined by key words and not as word-to-word as given in the model answer scheme. ) The model answer and the
More informationChem 102b Experiment 14: Part II Revised Preparation of Esters
http://www.chem.arizona.edu/courseweb/981/chem102b1/fisher_esterification.html Purpose of the Experiment: Chem 102b Experiment 14: Part II Revised Preparation of Esters Students will be given alcohols
More informationChemistry *P45044A0128* Pearson Edexcel P45044A
Write your name here Surname ther names Pearson Edexcel International Advanced Level entre Number andidate Number hemistry Advanced Unit 4: General Principles of hemistry I Rates, Equilibria and Further
More informationChem 1B Objective 7: Understand equilibrium reactions (equilibrium constant, LeChatelier s principle, equilibrium calculation).
Chem 1B Objective 7: Understand equilibrium reactions (equilibrium constant, LeChatelier s principle, equilibrium calculation). Key Ideas: Many important reactions are equilibrium reactions, e.g., many
More informationLecture 12. Complications and how to solve them
Lecture 12 Complications and how to solve them 1. Pseudo Order An expression for second order reaction 2A Products Can be written as, -da/dt = k [A] 2 And the integration, 1/A 2 da = kdt 1/A t 1/A o =
More informationGCSE Chemistry. Module C7 Further Chemistry: What you should know. Name: Science Group: Teacher:
GCSE Chemistry Module C7 Further Chemistry: What you should know Name: Science Group: Teacher: R.A.G. each of the statements to help focus your revision: R = Red: I don t know this A = Amber: I partly
More informationUses of GC/MS. Synthesis of 1-Bromobutane Butenes from 2-Butanol Fisher Esterification of Benzoic Acid Nitration of Methyl Benzoate
Instrument Uses of GC/MS 0 TechPrep Senior Event 0 Honors Project 0 Gasoline Analysis-General Chemistry 0 Ester Synthesis and Analysis-Chemistry for Liberal Arts Majors 0 Organic Reaction Product Analysis
More informationChapter 11: CHEMICAL KINETICS
Chapter : CHEMICAL KINETICS Study of the rate of a chemical reaction. Reaction Rate (fast or slow?) Igniting gasoline? Making of oil? Iron rusting? We know about speed (miles/hr). Speed Rate = changes
More informationA Unit Operations Lab Project that Combines the Concepts of Reactor Design and Transport Phenomena
Session #2313 A Unit Operations Lab Project that Combines the Concepts of Reactor Design and Transport Phenomena Benjamin J. Lawrence, Sundararajan V. Madihally, R. Russell Rhinehart School of Chemical
More information, by reacting CH 3 with ethanoic anhydride, (CH 3
1 A chemist prepares and analyses some esters. (a) The chemist prepares an ester of propan-2-ol, H 3 H(H)H 3, by reacting H 3 H(H)H 3 with ethanoic anhydride, (H 3 ) 2. Using structural formulae, write
More informationProjects for Organic Laboratory
1 Projects for rganic Laboratory Introduction For two lab periods in November, you will work on a project that requires you to design experiments, carry them out and interpret the results in order to reach
More informationTeaching Green Chemistry & Engineering Concepts in the Undergraduate Organic Laboratory via Biginelli and Hantzsch Reactions
Teaching Green Chemistry & Engineering Concepts in the Undergraduate rganic Laboratory via Biginelli and antzsch Reactions A.P. Dicks*, E. Aktoudianakis and S. Styler Department of Chemistry University
More informationAdvanced Unit 6: Chemistry Laboratory Skills II
Write your name here Surname Other names Pearson Edexcel International Advanced Level Centre Number Chemistry Advanced Unit 6: Chemistry Laboratory Skills II Candidate Number Thursday 16 January 2014 Morning
More informationChemical Kinetics. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Chemical Kinetics Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chemical Kinetics Thermodynamics does a reaction take place? Kinetics how fast does a reaction
More informationSAMPLE CHEMISTRY QUESTIONS MIXTURE OF UNIT 3 & 4 MATERIALS
SAMPLE CHEMISTRY QUESTIONS MIXTURE OF UNIT 3 & 4 MATERIALS QUESTION 1 The equation describing the production of butyl ethanoate is given below. Catalyst C4H 9OH CH 3COOH CH 3COOC 4H 9 H 2O( l ) 0.0500
More informationAP Chemistry - Notes - Chapter 12 - Kinetics Page 1 of 7 Chapter 12 outline : Chemical kinetics
AP Chemistry - Notes - Chapter 12 - Kinetics Page 1 of 7 Chapter 12 outline : Chemical kinetics A. Chemical Kinetics - chemistry of reaction rates 1. Reaction Rates a. Reaction rate- the change in concentration
More informationEXPERIMENT 7- SAPONIFICATION RATE OF TERT- BUTYL CHLORIDE
1 THEORY EXPERIMENT 7- SAPONIFICATION RATE OF TERT- BUTYL CHLORIDE The field of chemical kinetics is concerned with the rate or speed at which a chemical reaction occurs. Knowledge of a chemical reaction
More informationCHM 5423 Atmospheric Chemistry Notes on kinetics (Chapter 4)
CHM 5423 Atmospheric Chemistry Notes on kinetics (Chapter 4) Introduction A mechanism is one or a series of elementary reactions that convert reactants into products or otherwise model the chemistry of
More informationIn some cases, even an individual ester smells similar to a natural aroma. Some examples include:
What are Esters? Many of the compounds that contribute to the flavors and aromas in fruits and flowers are esters. Natural flavors and aromas result from complex mixtures of many compounds, esters being
More informationBiodiesel Fundamentals for High School Chemistry Classes. Laboratory 4: Chemical Equilibrium in Biodiesel
Laboratory 4: Chemical Equilibrium in Biodiesel Production Topics Covered Forward chemical reactions vs. reverse reactions Chemical reactions in equilibrium Ways to stimulate a reaction to proceed towards
More informationFriedel-Crafts Alkylation
Friedel-Crafts Alkylation Summary: The Friedel-Crafts alkylation reaction proceeds similarly to the acylation reaction, but uses an alkyl halide to attach an alkyl group to an aromatic ring. Anhydrous
More informationChapter 12. Chemical Kinetics
Chapter 12 Chemical Kinetics Chapter 12 Table of Contents 12.1 Reaction Rates 12.2 Rate Laws: An Introduction 12.3 Determining the Form of the Rate Law 12.4 The Integrated Rate Law 12.5 Reaction Mechanisms
More information1. Define molarity and give the symbol for this unit. Do the same for mass % (a.k.a. % w/w).
CHM 112 Study Guide I Chap 12-14 & 11.1 & 11.3 Sp 14 1. Closed book. Write your name on the back of the last page & your initials on the back of the other pages. 2. Show calculations and logic throughout
More informationCHAPTER 9 LECTURE NOTES
CHAPTER 9 LECTURE NOTES 9.1, 9.2: Rate of a reaction For a general reaction of the type A + 3B 2Y, the rates of consumption of A and B, and the rate of formation of Y are defined as follows: Rate of consumption
More informationChemical Kinetics. Rate = [B] t. Rate = [A] t. Chapter 12. Reaction Rates 01. Reaction Rates 02. Reaction Rates 03
Chapter Chemical Kinetics Reaction Rates 0 Reaction Rate: The change in the concentration of a reactant or a product with time (M/s). Reactant Products aa bb Rate = [A] t Rate = [B] t Reaction Rates 0
More informationwhere a + b = 2 (this is the general case) These all come from the fact that this is an overall second order reaction.
Chapter 7 Problems Page of 6 //007 7. Hydrolysis of ethyl acetate is as follows: EtAc + OH - Ac - + EtOH. At 5 ºC, the disappearance of OH - is used to determine the extent of the reaction, leading to
More informationProf. Jason Kahn University of Maryland, College Park Your SID #: General Chemistry and Energetics Final Exam (150 points total) December 19, 2016
Chemistry 134 Your Name: Prof. Jason Kahn University of Maryland, College Park Your SID #: General Chemistry and Energetics Final Exam (150 points total) December 19, 2016 You have 120 minutes for this
More informationAlcohols, Phenols and Ethers
SUBJECTIVE PROBLEMS: Alcohols, Phenols and Ethers Q1. An organic liquid (A), containing C, H and O with boiling point: 78 o C, and possessing a rather pleasant odour, on heating with concentrated sulphuric
More informationChapter 14 Chemical Kinetics
4//004 Chapter 4 Chemical Kinetics 4- Rates of Chemical Reactions 4- Reaction Rates and Concentrations 4-3 The Dependence of Concentrations on Time 4-4 Reaction Mechanisms 4-5 Reaction Mechanism and Rate
More informationALE 9. Equilibrium Problems: ICE Practice!
Name Chem 163 Section: Team Number: ALE 9. Equilibrium Problems: ICE Practice! (Reference: 17.5 Silberberg 5 th edition) Equilibrium Calculations: Show all work with correct significant figures. Circle
More informationChemical Kinetics. Reaction rate and activation energy of the acid hydrolysis of ethyl acetate LEC 05. What you need: What you can learn about
LEC 05 Chemical Kinetics Reaction rate and activation energy of the acid hydrolysis What you can learn about Reaction rate Rate law for first and second order reactions Reactions with pseudo-order Arrhenius
More informationFRONT PAGE FORMULA SHEET - TEAR OFF
FRONT PAGE FORMULA SHEET - TEAR OFF N A = 6.022 x 10 23 C = ( 5 / 9 ) ( F - 32) F = ( 9 / 5 )( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013
More informationReactors. Reaction Classifications
Reactors Reactions are usually the heart of the chemical processes in which relatively cheap raw materials are converted to more economically favorable products. In other cases, reactions play essential
More informationKinetics Practice Test 2017 Name: date: 1. Use the data provided the answer the question.
Kinetics Practice Test 2017 Name: date: 1. Use the data provided the answer the question. The data above was obtained for a reaction in which X + Y Z. Which of the following is the rate law for the reaction?
More informationChemistry 102 Spring 2017 Discussion #13, Chapter 17 Student name TA name Section. Things you should know when you leave Discussion today: ( G o f
Chemistry 0 Spring 07 Discussion #3, Chapter 7 Student name TA name Section Things you should know when you leave Discussion today:. ΔSsys = ΔrS = Σ [ni (S )]product - Σ [nj (S )]reactants. ΔGº = -T ΔSnet
More informationPhysical Chemistry Chapter 6 Chemical Kinetics
Physical Chemistry Chapter 6 Chemical Kinetics by Azizul Helmi Sofian Faculty of Chemical & Natural Resources Engineering azizulh@ump.edu.my Chapter Description Aims To define rate laws accordingly To
More informationCh 13 Chemical Kinetics. Modified by Dr. Cheng-Yu Lai
Ch 13 Chemical Kinetics Modified by Dr. Cheng-Yu Lai Outline 1. Meaning of reaction rate 2. Reaction rate and concentration 3. Writing a Rate Law 4. Reactant concentration and time 5. Reaction rate and
More informationChem 6 Sample exam 1 (150 points total) NAME:
Chem 6 Sample exam 1 (150 points total) @ This is a closed book exam to which the Honor Principle applies. @ The last page contains equations and physical constants; you can detach it for easy reference.
More informationLAB 17: SYNTHESIS OF BANANA OIL: REACTIONS OF ALCOHOLS: FISCHER ESTERIFICATION
LAB 17: SYNTESIS F BANANA IL: REATINS F ALLS: FISER ESTERIFIATIN PURPSE: To synthesize isoamyl acetate by Fischer Esterification. To purify a liquid by simple distillation. SAFETY NERNS: Always wear safety
More informationBAE 820 Physical Principles of Environmental Systems
BAE 820 Physical Principles of Environmental Systems Acquisition of reaction rate data Dr. Zifei Liu Uncertainties in real world reaction rate data Most interesting reaction systems involves multiple reactions,
More informationIt must be determined from experimental data, which is presented in table form.
Unit 10 Kinetics The rate law for a reaction describes the dependence of the initial rate of a reaction on the concentrations of its reactants. It includes the Arrhenius constant, k, which takes into account
More informationDETERMINATION OF ACETIC ACID IN VINEGAR
DETERMINATION OF ACETIC ACID IN VINEGAR 1 INTRODUCTION Juices from plants and fruits contain sugar. When these juices are fermented, the sugar molecules are converted into ethyl alcohol molecules (C 2
More informationCHEM4. General Certificate of Education Advanced Level Examination June Unit 4 Kinetics, Equilibria and Organic Chemistry
Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials General Certificate of Education Advanced Level Examination June 2010 Question 1 2 Mark Chemistry
More informationExperimental Procedure Lab 402
Experimental Procedure Lab 402 Overview Measured volume of several solutions having known concentrations of reactants are mixed in a series of trials. The time required for a visible color change to appear
More informationName. Department of Chemistry SUNY/Oneonta. Chem Organic Chemistry II Examination #3 - March 31, 2003
INSTRUTINS Name Department of hemistry SUNY/neonta hem 322 - rganic hemistry II Examination #3 - March 31, 2003 This examination has two parts. Part I is in multiple choice format and the answers should
More informationMSc course Adsorption, Kinetics & Catalysis
MSc course Adsorption, Kinetics & Catalysis Kinetics Chapter.-.6 Prof. Fran de Groot MSc Nanomaterials Chemistry and Physics Utrecht University master / University of Nijmegen / 987 / Theoretical Chemistry
More information12A Lab Activity Notes
12A Lab Activity Notes Lab Activity 12 In this experiment, RX reacts with a base. The methoxide ion (CH 3 O - ) is a small, strong base. The tert-butoxide ion ((CH 3 ) 3 CO - ) is a large, strong base.
More informationLecture 15. Unimolecular reactions
Lecture 15 Unimolecular reactions How do they occur? Look at the following reaction. Sir Cyril Hinshelwood 1897-1967, Nobel 1956 Cyclo-C 3 H 6 CH 3 -CH=CH 2, the rate = k[cyclo-c 3 H 6 ] These are unimolecular
More informationName:. Correct Questions = Wrong Questions =.. Unattempt Questions = Marks =
Name:. Correct Questions = Wrong Questions =.. Unattempt Questions = Marks = 1. Which salt is colorless? (A) KMn 4 (B) BaS 4 (C) Na 2 Cr 4 (D) CoCl 2 2. Which 0.10 M aqueous solution exhibits the lowest
More informationOH [H + ] KMnO 4 DME OH
1.a. Reaction 1 is an elimination reaction which includes a rearrangement via a hydride shift. Reaction 2 is an oxidation reaction that leads to a cis-diol. This reaction was used to qualitatively confirm
More informationChemistry 1B Experiment 17 89
Chemistry 1B Experiment 17 89 17 Thermodynamics of Borax Solubility Introduction In this experiment, you will determine the values of H and S for the reaction which occurs when borax (sodium tetraborate
More informationExp t 83 Synthesis of Benzyl Acetate from Acetic Anhydride
Exp t 83 Synthesis of Benzyl Acetate from Acetic Anhydride from K. L. Williamson, Macroscale and Microscale rganic Experiments, 2nd Ed. 1994, Houghton Mifflin, Boston p385; revised Prelab Exercise: 10/14/00
More informationChapter 14 Chemical Kinetics
Chapter 14 Chemical Kinetics Factors that Affect Reaction rates Reaction Rates Concentration and Rate The Change of Concentration with Time Temperature and Rate Reactions Mechanisms Catalysis Chemical
More informationCh 13 Rates of Reaction (Chemical Kinetics)
Ch 13 Rates of Reaction (Chemical Kinetics) Reaction Rates and Kinetics - The reaction rate is how fast reactants are converted to products. - Chemical kinetics is the study of reaction rates. Kinetics
More informationFor this lab, you will determine the purity of the aspirin by titration and by spectrophotometric analysis.
Introduction: ommercially prepared aspirin tablets are not considered 100% pure acetylsalicylic acid. Most aspirin tablets contain a small amount of binder which helps prevent the tablets from crumbling.
More informationBioinformatics: Network Analysis
Bioinformatics: Network Analysis Reaction Kinetics COMP 572 (BIOS 572 / BIOE 564) - Fall 2013 Luay Nakhleh, Rice University 1 Reaction kinetics is the study of how fast chemical reactions take place, what
More informationPRODUCTION OF ETHYL ACETATE USING CATALYTIC REACTION METHOD
PRODUCTION OF ETHYL ACETATE USING CATALYTIC REACTION METHOD Bamunusingha Arachchige Nadeeka Niroshinie Bamunusingha (108001 T) Thesis submitted in partial fulfillment of the requirements for the degree
More informationThe Atom, The Mole & Stoichiometry. Chapter 2 I. The Atomic Theory A. proposed the modern atomic model to explain the laws of chemical combination.
Unit 2: The Atom, The Mole & Stoichiometry Chapter 2 I. The Atomic Theory A. proposed the modern atomic model to explain the laws of chemical combination. Postulates of the atomic theory: 1. All matter
More informationChapter 13 Lecture Lecture Presentation. Chapter 13. Chemical Kinetics. Sherril Soman Grand Valley State University Pearson Education, Inc.
Chapter 13 Lecture Lecture Presentation Chapter 13 Chemical Kinetics Sherril Soman Grand Valley State University Ectotherms Lizards, and other cold-blooded creatures, are ectotherms animals whose body
More informationChemistry 12 Dr. Kline 28 September 2005 Name
Test 1 first letter of last name Chemistry 12 Dr. Kline 28 September 2005 Name This test consists of a combination of multiple choice and other questions. There should be a total of 24 questions on 8 pages;
More informationExperiment 2: The Rate of an Iodine Clock Reaction
Experiment 2: The Rate of an Iodine Clock Reaction Introduction: Some reactions, including most of the ones that you have seen before, occur so rapidly that they are over as soon as the reactants are mixed.
More informationClass Results Simulator:
Class Results http://chemconnections.org/general/chem120/equil-graph.html Simulator: http://chemconnections.org/java/equilibrium/ http://chemconnections.org/general/chem120/equil-graph.html The changes
More informationGeneral Chemistry II FINAL EXAMINATION
General Chemistry II 141 FINAL EXAMINATIN PART I ( points each) CHEM 141 (Fall 009) Version AF09 Multiple choice - scantron. Please D NT write or mark on this paper. Write your correct answer on 1. Which
More informationNuclear Engineering Jordan University of Science and Technology Faculty of Engineering Department of Nuclear Engineering
Nuclear Jordan University of Science and Technology Faculty of Department of Nuclear Undergraduate Curriculum for the Bachelor Degree in Nuclear (2013) 1 Nuclear Study Plan First Year CIS 100 Computer
More informationCHEM4. General Certificate of Education Advanced Level Examination June Unit 4 Kinetics, Equilibria and Organic Chemistry
Centre Number Surname Candidate Number For Examiner s Use ther Names Candidate Signature Examiner s Initials General Certificate of Education Advanced Level Examination June 2012 Question 1 2 Mark Chemistry
More informationAdvanced Physical Chemistry CHAPTER 18 ELEMENTARY CHEMICAL KINETICS
Experimental Kinetics and Gas Phase Reactions Advanced Physical Chemistry CHAPTER 18 ELEMENTARY CHEMICAL KINETICS Professor Angelo R. Rossi http://homepages.uconn.edu/rossi Department of Chemistry, Room
More information7/30/07 MIKE HALL ALKENE FORMATION: ACID-CATALYZED DEHYDRATION OF AN ALCOHOL
EXPERIMENT #5 GRACE KIM 7/30/07 MIKE ALL ALKENE FRMATIN: ACID-CATALYZED DEYDRATIN F AN ALCL 2. INTRDUCTIN AND PURPSE 2-methylcyclohexanol was converted to a mixture of 1-methyl and 3-methylcyclohexene
More informationModule overview. The approach. Practical work. ICT resources. The topics. Skills assessment. Health and safety. Advance preparation
Module overview The approach This module is equivalent in extent to three of the earlier modules C1 C3 or C4 C6. There are three broad aims: to extend the coverage of key themes in modern chemistry (organic
More informationModeling and Simulation of Temperature Profiles in a Reactive Distillation System for Esterification of Acetic Anhydride with Methanol
Modeling and Simulation of Temperature Profiles in a Reactive Distillation System for Esterification of Acetic Anhydride with Methanol N.Asiedu *, D.Hildebrandt *, D.Glasser * Centre of Material and Process
More informationCOURSE OUTLINE. COURSE NUMBER: SCI 502 WRITTEN / REVISED: September, 2011 LEVEL OF COURSE: AP NUMBER OF CREDITS: SIX (6)
COURSE OUTLINE NAME OF COURSE: CHEMISTRY COURSE NUMBER: SCI 502 WRITTEN / REVISED: September, 2011 LEVEL OF COURSE: AP NUMBER OF CREDITS: SIX (6) PREREQUISITES: Honors Chemistry or qualifying test. Concurrent
More informationCHE 113 MIDTERM EXAMINATION October 25, 2012
CHE 113 MIDTERM EXAMINATION October 25, 2012 University of Kentucky Department of Chemistry READ THESE DIRECTIONS CAREFULLY BEFORE STARTING THE EXAMINATION! It is extremely important that you fill in the
More informationOverarching Big Ideas, Enduring Understandings, and Essential Questions (These spiral throughout the entire curriculum.)
Course: Honors Chemistry Grade: 10-12 Designer(s): M. Rush Overview of Course (Briefly describe what students should understand and be able to do as a result of engaging in this course): This course is
More informationChapter 11 Rate of Reaction
William L Masterton Cecile N. Hurley http://academic.cengage.com/chemistry/masterton Chapter 11 Rate of Reaction Edward J. Neth University of Connecticut Outline 1. Meaning of reaction rate 2. Reaction
More informationTOPIC 6: Chemical kinetics
TOPIC 6: Chemical kinetics Reaction rates Reaction rate laws Integrated reaction rate laws Reaction mechanism Kinetic theories Arrhenius law Catalysis Enzimatic catalysis Fuente: Cedre http://loincognito.-iles.wordpress.com/202/04/titanic-
More informationCHEM 1412 SAMPLE FINAL EXAM
CHEM 1412 SAMPLE FINAL EXAM PART I - Multiple Choice (2 points each) 1. In which colligative property(ies) does the value decrease as more solute is added? A. boiling point B. freezing point and osmotic
More information8. The table below describes two different reactions in which Reaction 1 is faster. What accounts for this observation? Reaction 1 Reaction 2.
Public Review - Rates and Equilibrium June 2005 1. What does X represent in the diagram below? (A) activation energy for the forward reaction (B) activation energy for the reverse reaction (C) heat of
More informationGreen Chemistry in the Undergraduate Organic Laboratory: Microwave-Assisted Synthesis of a Natural Insecticide on Basic Montmorillonite K10 Clay
LAB PRCEDURE: Green Chemistry in the Undergraduate rganic Laboratory: Microwave-Assisted Synthesis of a Natural Insecticide on Basic Montmorillonite K10 Clay Matthew R. Dintzner*, Paul R. Wucka and Thomas
More informationMultistep Synthesis of 5-isopropyl-1,3-cyclohexanedione
Multistep Synthesis of 5-isopropyl-1,3-cyclohexanedione The purpose of this experiment was to synthesize 5-isopropyl-1,3-cyclohexanedione from commercially available compounds. To do this, acetone and
More informationChapter 12. Chemical Kinetics
Chapter 12 Chemical Kinetics Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section
More information11/2/ and the not so familiar. Chemical kinetics is the study of how fast reactions take place.
Familiar Kinetics...and the not so familiar Reaction Rates Chemical kinetics is the study of how fast reactions take place. Some happen almost instantaneously, while others can take millions of years.
More informationESTERIFICATION OF PHTHALIC ANHYDRIDE WITH 2-ETHYLHEXANOL
ESTERIFICATION OF PHTHALIC ANHYDRIDE WITH 2-ETHYLHEXANOL Satchidanand R Satpute 1, Yogesh H Shinde 2, Prakash V Chavan 1 * 1 Department of Chemical Engineering, College of Engineering, Bharati Vidyapeeth
More information4023 Synthesis of cyclopentanone-2-carboxylic acid ethyl ester from adipic acid diethyl ester
NP 4023 Synthesis of cyclopentanone-2-carboxylic acid ethyl ester from adipic acid diethyl ester NaEt C 10 H 18 4 Na C 2 H 6 C 8 H 12 3 (202.2) (23.0) (46.1) (156.2) Classification Reaction types and substance
More informationCHAPTER 12 CHEMICAL KINETICS
5/9/202 CHAPTER 2 CHEMICAL KINETICS CHM52 GCC Kinetics Some chemical reactions occur almost instantaneously, while others are very slow. Chemical Kinetics - study of factors that affect how fast a reaction
More informationEquilibrium. Reversible Reactions. Chemical Equilibrium
Equilibrium Reversible Reactions Chemical Equilibrium Equilibrium Constant Reaction Quotient Le Chatelier s Principle Reversible Reactions In most chemical reactions, the chemical reaction can be reversed,
More informationSummer Assignment for AP Chemistry: I hope you are all ready for a fun, yet challenging year. You have a good foundation in basic chemistry from Chem
Summer Assignment for AP Chemistry: I hope you are all ready for a fun, yet challenging year. You have a good foundation in basic chemistry from Chem 1, but AP Chem will be a little different. Rather than
More informationIn a forward reaction, the reactants collide to produce products and it goes from left to
Worksheet #1 Approaching Equilibrium Read unit II your textbook. Answer all of the questions. Do not start the questions until you have completed the reading. Be prepared to discuss your answers next period.
More information