Chemical Kinetics Ziyue Zhu 2015/2/4
|
|
- Helen Manning
- 5 years ago
- Views:
Transcription
1 Chemical Kinetics Ziyue Zhu 2015/2/4
2 Introduction: The purpose of this experiment was to measure the effects of changes in the concentrations of reactants and temperature on the rate of a reaction. The definition of reaction rate is: the amount of reagent (conventionally reported in units of molarity) consumed or produced per unit of time Rate = - Δ[reactant]/Δt = Δ[product]/Δt (1) Effects of concentration on reaction rate can be mathematically summarized by a rate law: Rate = -Δ[A]/Δt = k[a] 1 [B] 1 (2) The rate law often has the form: Rate= k[a] x [B] y [C] z (3) Effects of a temperature Change on the Reaction Rate: K = Ae -Ea*/RT (4) The first step of this experiment was to run three qualitative tests before the measurements began. In the first step, a few drops of H2O2 was added into KI solution and the following reaction would occur: H2O2 + 2I - +2H + I2 + 2H2O (5) The second test was to divide the mixture into three portion and add a few drops of starch solution into the second portion. Finally, thiosulfate solution and a few starch was added into the third portions and the following reaction will occur: 2S2O I2 2I - + S4O6 2- (6) Take record of observations after each test was finished. The second step of this experiment was to measure the effects of concentration and temperature on the rate of reactions. The first step was to mix D.I. Water, Buffer, Na2S2O3, KI and starch for A-H measurements with different given volumes. Then poured H2O2 and take record of time from the moments H2O2 was poured to the moment the solution began to change color because the reaction (5) and (6) happened. In that case, the time could be used to calculate the rate of reaction by using equation (2). In addition, measurements E and H would need to record temperature and the temperature of measurements H should always be 5 o C lower than the temperature of measurements E. In that case, it was easy to tell the effects of temperature on the rate of reaction by comparing measurements E with H.
3 Data and Calculations Table 1: Molar concentrations of reagent solutions: Reagents S2O3 2- I - H2O M 0.06M 0.11M Concentrations Table 2: Data summary table Sol n Temp [I - ] Log[I - ] [H2O2] log[h2o2] Δt min Rate: -Δ[H2O2]/Δt log(rate) A x x B x x C 9x x x D 6x x x E 22 o C 6x x F 6x x G 6x x H 17 o C 6x x
4 Calculations: 1. a. Moles S2O3 2 in each solution. 9.5x10-5 mol (a). b. Number of moles of I2 required to exhaust the moles of S2O3 2 from 4.75x10-5 mol c. Number of moles of H2O2 required to produce number of moles of I2 in (b). 4.75x10-5 mol d. Change in H2O2 concentration, Δ [H2O2] The number of moles of H2O2 lost (from c above) IS the negative change in moles of H2O2 ( Δ moles H2O2). You just need to change moles to molarity (what is final solution volume?) 4.75x10-4 M (Note: Answers to a, b, c, and d are identical for all eight solutions.)
5 2. Reaction Order (attach graphs): Graph 1 : determining r, the order in HxOx: Graph 2: determining s, the order in I -: According to the two graph above, it is easily to tell the value of r and s. r = s =
6 3. Value of rate constant, k Run k A B C D E F G Average The units should be mol x L x min -1 Using the data above, Ea* = and units should be J/ (Δmol x o C) All the calculations are on the carbon copy of the calculation page.
7 Results and discussion: First of all, the results of the qualitative tests were: only the second portion turned to blue color. The reason why the first test did not change color was because that the H2O2 can change the I - into I2. However, I2 did not has much color in water when it was diluted. In the second test, the starch was added into the solution and OH group in starch reacted with I2 and formed some clathrate solution which could only relfect blue light so that the solution showed blue color. In the third test, the thiosulfate solution was added first and the S2O3 2- reacted with I2 and consumed all of I2 so that when the starch was added after the first step, no I2 was left to react with starch. In that case, the solution did not change into blue. The results of r value was and the s value was ,according to graph 1 and 2.The two graph shows that the log(rate) has a linear relation with log(h2o2) and log(i - ). These means the reaction order in H2O2 and I - was both in 1 st order. The expected value of r and s are both 1 so the error percentage of r was 16.26% and s was 28.68%. The results of k value was in average. This means that the reaction rate constant was mol per L per min. Because the expected k value was not found, the error percentage can not be calculated. The value of Ea* was J per Δmoles per minute. The most possible reason of the errors was that during the F trials, the starch was not added before the time was recorded. In that case, the Δt of trial F was higher than actual Δt. Another possible reason was when doing several trails, the actual compounds added into the solution was not as accurate as the given table. Post-Lab Questions: 1. The reason of the errors caused the actual value of r and s lower than 1 because if the starch was added later, it would let the Δt increase so that the rate of reaction will slow down. In that case, the log(rate) will be lower than expected value and the r and s value would also be lower. 2. According to the data of experiment, the rate of reaction was increased when the concentration of the reactants was increased. The rate of reaction was decreased when the temperature of the reaction was decreased. This two conclusion happened when the k value was determined to be 1 or close to 1.
Rate Properties of an Iodide Oxidation Reaction
Rate Properties of an Iodide Oxidation Reaction GOAL AND OVERVIEW The rate law for the reduction reaction of peroxodisulfate (PODS) by iodide: S 2 O8 2 (aq) + 2 I (aq) I 2 (aq) + 2 SO4 2 (aq) will be determined.
More informationLowell High School AP Chemistry Spring 2009 REACTION KINETICS EXPERIMENT
Lowell High School AP Chemistry Spring 2009 REACTION KINETICS EXPERIMENT Complete the following for Pre-Lab on a clean sheet of paper: (1) In your own words, explain the following: a. why the I 2 concentration
More informationA Clock Reaction: Determination of the Rate Law for a Reaction
1 A Clock Reaction: Determination of the Rate Law for a Reaction This experiment involves the study of the rate properties, or chemical kinetics, of the following reaction between iodide ion and bromate
More informationInvestigating the Effect of Concentration on an Iodide Persulphate Reaction, and Rate Law Determination. Lab Performed on Monday, February 25 th, 2013
Investigating the Effect of Concentration on an Iodide Persulphate Reaction, and Rate aw Determination ab Performed on Monday, February 25 th, 2013 Introduction The purpose of this lab is to observe the
More informationDetermining the Rate Law for a Chemical Reaction
Determining the Rate Law for a Chemical Reaction Purpose: To determine the reaction orders, rate law, and rate constant for the reaction between persulfate ions, SO8 -, and iodide ions, I - Introduction
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 informationEXPERIMENT 1 REACTION RATE, RATE LAW, AND ACTIVATION ENERGY THE IODINE CLOCK REACTION
PURPOSE: To determine the Rate Law and the Activation Energy for a reaction from experimental data. PRINCIPLES: The Rate Law is a mathematical expression that predicts the rate of a reaction from the concentration
More informationExperiment 26 - Kinetics
Chem 1B Dr. White 175 Experiment 26 - Kinetics Objectives To determine the rate law for the reaction between iodide and bromate under acidic conditions To investigate the effect of temperature on rate
More informationKinetics of an Iodine Clock Reaction
Kinetics of an Iodine Clock Reaction Introduction: In this experiment, you will determine the rate law for a reaction and the effect of concentration on the rate of the reaction by studying the initial
More informationKinetics of an Iodine Clock Reaction
Kinetics of an Iodine Clock Reaction Introduction: In this experiment, you will determine the rate law for a reaction and the effect of concentration on the rate of the reaction by studying the initial
More informationIODINE CLOCK REACTION KINETICS
Name: Section Chemistry 104 Laboratory University of Massachusetts Boston IODINE CLOCK REACTION KINETICS PRELAB ASSIGNMENT Calculate the initial concentration of H 2 O 2 that exists immediately after mixing
More informationTHE EFFECT OF TEMPERATURE AND CONCENTRATION ON REACTION RATE
THE EFFECT OF TEMPERATURE AND CONCENTRATION ON REACTION RATE INTRODUCTION FACTORS INFLUENCING REACTION RATE: The study of chemical reactions is not complete without a consideration of the rates at which
More informationKinetics of an Iodine Clock Reaction Lab_Student Copy
Kinetics of an Iodine Clock Reaction Lab_Student Copy Purpose: Purpose: In this lab, you will find the reaction rate, rate law,, and observe the effects of a catalyst for the oxidation of iodide ions by
More informationThe rate equation relates mathematically the rate of reaction to the concentration of the reactants.
1.9 Rate Equations Rate Equations The rate equation relates mathematically the rate of reaction to the concentration of the reactants. For the following reaction, aa + bb products, the generalised rate
More informationPURPOSE: To determine the Rate Law for the following chemical reaction:
PURPOSE: To determine the Rate Law for the following chemical reaction: H 2 O 2 (aq) + 2 I - (aq) + 2 H 3 O + (aq) 4 H 2 O(l) + I 2 (aq) Hydrogen Iodide Hydronium Water Iodine Peroxide Ion Ion PRINCIPLES:
More informationCHM112 Lab Iodine Clock Reaction Part 2 Grading Rubric
Name Team Name CHM112 Lab Iodine Clock Reaction Part 2 Grading Rubric Criteria Points possible Points earned Lab Performance Printed lab handout and rubric was brought to lab 3 Initial concentrations completed
More informationKinetics of an Iodine Clock Reaction Lab_ Teacher s Key
Kinetics of an Iodine Clock Reaction Lab_ Teacher s Key Purpose: In this lab, you will find the reaction rate, rate law,, and observe the effects of a catalyst for the oxidation of iodide ions by bromate
More information#5 Chemical Kinetics: Iodine Clock Reaction
#5 Chemical Kinetics: Iodine Clock Reaction In the previous experiment, we discussed the factors that influence the rate of a chemical reaction and presented the terminology used in quantitative relations
More informationChem 401 Unit 1 (Kinetics & Thermo) Review
KINETICS 1. For the equation 2 H 2(g) + O 2(g) 2 H 2 O (g) How is the rate of formation of H 2 O mathematically related to the rate of disappearance of O 2? 1 Δ [H2O] Δ[O 2] = 2 Δt Δt 2. Determine the
More informationTHE EFFECT OF TEMPERATURE AND CONCENTRATION ON REACTION RATE
THE EFFECT OF TEMPERATURE AND CONCENTRATION ON REACTION RATE INTRODUCTION FACTORS INFLUENCING REACTION RATE: The study of chemical reactions is not complete without a consideration of the rates at which
More informationExamining the Effect of Temperature on Reaction Rate
1 Purpose: To measure reaction rate at different temperatures for the reaction between persulfate ions, S2O8-2, and iodide ions, I -, and thereby determine the activation energy and frequency factor for
More informationKinetics; A Clock Reaction
Kinetics; A Clock Reaction Background This experiment involves the study of the rate properties, or chemical kinetics, of the following reaction between iodide ion (I - ) and bromate ion (BrO 3 - ) under
More informationExperiment 2: Factors Affecting Reaction Rates
Objective: Part A To determine the effect of concentration on the rate of formation of Iodine, I 2, and therefore, determine the reaction s rate law. Part B To study the effect of temperature on the rate
More informationWhen a solution of thiosulfate is acidified, the following reaction takes place: S2O3 2 - (aq) + 2H + (aq) H2O + SO2 (g) + S (s) (1)
EXPERIMENT 1 The Kinetics of a Thiosulfate Solution INTRODUCTION: Various approaches are used to study the kinetics of reactions. A usual procedure is to monitor some property, such as intensity of color
More informationLab #5 - Limiting Reagent
Objective Chesapeake Campus Chemistry 111 Laboratory Lab #5 - Limiting Reagent Use stoichiometry to determine the limiting reactant. Calculate the theoretical yield. Calculate the percent yield of a reaction.
More informationCHM112 Lab Iodine Clock Reaction Part 1 Grading Rubric
Name Team Name CHM112 Lab Iodine Clock Reaction Part 1 Grading Rubric Criteria Points possible Points earned Lab Performance Printed lab handout and rubric was brought to lab 3 Initial concentrations completed
More informationStoichiometry. Please take out your notebooks
Stoichiometry Please take out your notebooks Stoichiometry stochio = Greek for element metry = measurement Stoichiometry is about measuring the amounts of elements and compounds involved in a reaction.
More informationExperiment #5. Iodine Clock Reaction Part 1
Experiment #5. Iodine Clock Reaction Part 1 Introduction In this experiment you will determine the Rate Law for the following oxidation- reduction reaction: 2 H + (aq) + 2 I (aq) + H 2 O 2 (aq) I 2 (aq)
More informationCONSIDER THE FOLLOWING REACTIONS
CONSIDER THE FOLLOWING REACTIONS BaCl 2 + MgSO 4 BaSO 4 + MgCl 2 2KI + Pb(NO3)2 PbI2 + 2KNO3 Fe + H20 (g) Fe2O3 + H2 All reactions have two reactants yielding the reaction. WHAT IS A LIMITING REACTANT?
More informationUNIT 2: KINETICS RATES of Chemical Reactions (TEXT: Chap 13-pg 573)
UNIT 2: KINETICS RATES of Chemical Reactions (TEXT: Chap 13-pg 573) UNIT 2: LAB 1. A Brief Introductory Kinetics Investigation A) Set up 4 test tubes containing about 5 ml of 0.1 M sodium oxalate sol n.
More informationCHAPTER 13 (MOORE) CHEMICAL KINETICS: RATES AND MECHANISMS OF CHEMICAL REACTIONS
CHAPTER 13 (MOORE) CHEMICAL KINETICS: RATES AND MECHANISMS OF CHEMICAL REACTIONS This chapter deals with reaction rates, or how fast chemical reactions occur. Reaction rates vary greatly some are very
More informationCHEMISTRY - CLUTCH CH.13 - CHEMICAL KINETICS.
!! www.clutchprep.com CONCEPT: RATES OF CHEMICAL REACTIONS is the study of reaction rates, and tells us the change in concentrations of reactants or products over a period of time. Although a chemical
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 informationMaking Buffers v010417
Making Buffers v010417 Purposes of the Experiment Make a buffer with a desired ph. Demonstrate the buffering capacity of this buffer. Background Buffers are solutions containing a mixture of a weak acid
More informationGoal: During this lab students will gain a quantitative understanding of limiting reagents.
LIMITING REAGENT LAB: THE REACTION BETWEEN VINEGAR AND BAKING SODA Goal: During this lab students will gain a quantitative understanding of limiting reagents. Safety: Safety goggles should be worn at all
More informationChemistry 40S Chemical Kinetics (This unit has been adapted from
Chemistry 40S Chemical Kinetics (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 2 Lesson 1: Introduction to Kinetics Goals: Identify variables used to monitor reaction rate. Formulate
More informationRate of Reaction. Introduction
5 Rate of Reaction Introduction This experiment will allow you to study the effects of concentration, temperature, and catalysts on a reaction rate. The reaction whose rate you will study is the oxidation
More informationA Chemical Clock. 5. Consider each of the following questions regarding data and measurements:
A Chemical Clock Things to Consider 1. What are the three major objectives of this experiment? What methods will you try using to achieve each of these three objectives? 2. What is difference between reaction
More informationChem 401 Unit 1 (Kinetics & Thermo) Review
KINETICS 1. For the equation 2 H 2(g) + O 2(g) 2 H 2 O (g) How is the rate of formation of H 2 O mathematically related to the rate of disappearance of O 2? 2. Determine the relative reaction rates of
More informationName: Date: AP Chemistry. Titrations - Volumetric Analysis. Steps for Solving Titration Problems
Name: Date: AP Chemistry Titrations - Volumetric Analysis Term Volumetric analysis Burette Pipette titrate titre aliquot end point equivalence point indicator primary standard standardisation secondary
More informationExperiment 7 Can You Slow It Down?
Experiment 7 Can You Slow It Down? OUTCOMES After completing this experiment, the student should be able to: tell which factors influence the reaction rate and how they influence the rate. change the temperature
More informationUnit The mw of Na 2 CO 3 is : Na=23, O=16, C=12 A) 140 B) 106 C) 96 D) 100 E) 60
Unit 2 1- The mw of Na 2 CO 3 is : Na=23, O=16, C=12 A) 140 B) 106 C) 96 D) 100 E) 60 2- How many grams of Na 2 CO 3 (mw = 106 ) A) 318 B) 0.028 C) 134 D) 201 E) 67 in 3 moles, 3- Calculate the normal
More informationThe rate of reaction is defined as the change in concentration of a substance in unit time Its usual unit is mol dm -3 s -1
16. Kinetics II The rate of reaction is defined as the change in concentration of a substance in unit time Its usual unit is mol dm -3 s -1 When a graph of concentration of reactant is plotted vs time,
More informationExp. 2: The Superconductor YBa 2 Cu 3 O 7 (Text #1)
Exp. 2: The 1-2-3 Superconductor YBa 2 Cu 3 O 7 (Text #1) Last week: Performed high-temperature, solid-state reaction to prepare YBa 2 Cu 3 O x Thursday: Determine product stoichiometry ( x ) based on
More informationThe rate equation relates mathematically the rate of reaction to the concentration of the reactants.
1.9 Rate Equations Rate Equations The rate equation relates mathematically the rate of reaction to the concentration of the reactants. For the following reaction, aa + bb products, the generalised rate
More informationB. Activation Energy: Ea
B. Activation Energy: Ea a) Example reaction: the burning of charcoal in the BBQ C (s) + O 2(g) CO 2 (remember, burning is VERY exothermic) Question: Will charcoal in your BBQ spontaneously catch fire?
More informationEdexcel Chemistry A-level
Edexcel Chemistry A-level Topic 5 - Formulae, Equations and Amounts of Substance Flashcards What is the symbol for amount of substance? What is the symbol for amount of substance? n What is the unit used
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 informationIodine Clock Part I Chemical Kinetics
Collect: Iodine Clock Part I Chemical Kinetics (2015/11/17 revised) 50 ml Erlenmeyer flask (10): wash clean, dry, and cool 5 ml graduated pipet (2), pipet filler (1) Cork stopper (6) Stopwatch (1) (given
More informationEquilibrium. Why? Model 1 A Reversible Reaction. At what point is a reversible reaction completed?
Why? Equilibrium At what point is a reversible reaction completed? Most of the reactions that we have studied this year have been forward reactions once the reactant has changed into the product it stays
More informationWhat Is the Rate Law for the Reaction Between Hydrochloric Acid and Sodium Thiosulfate?
What Is the Rate Law for the Reaction Between Hydrochloric Acid and Sodium Thiosulfate? Introduction The collision theory of reactions suggests that the rate of a reaction depends on three important factors.
More informationName. Chem 116 Sample Examination #2
page 1 of 8 Name Last 5 digits of Student Number: XXX X Chem 116 Sample Examination #2 This exam consists of eight (8) pages, including this cover page. Be sure your copy is complete before beginning your
More informationExperiment 4: Rates of Chemical Reactions II: Kinetic Study of the Reaction between Ferric and Iodine Ions
Experiment 4: Rates of Chemical Reactions II: Kinetic Study of the Reaction between Ferric and Iodine Ions PURPOSE: To study kinetics of the reaction between ferric (Fe 3+ ) and iodide (I - ) ions, i.e.
More information, but bursts into flames in pure oxygen.
Chemical Kinetics Chemical kinetics is concerned with the speeds, or rates of chemical reactions Chemical kinetics is a subject of broad importance. How quickly a medicine can work The balance of ozone
More informationAcid-Base Titration Lab
Acid-Base Titration Lab Name Objectives: - To apply knowledge of molarity to properly dilute a concentrated base - To apply knowledge of solution stoichiometry in order to correctly determine the unknown
More informationTo see how this data can be used, follow the titration of hydrofluoric acid against sodium hydroxide:
Weak Acid Titration v010516 You are encouraged to carefully read the following sections in Tro (3 rd ed.) to prepare for this experiment: Sec 4.8, pp 168-174 (Acid/Base Titrations), Sec 16.4, pp 769-783
More informationU N I T T E S T P R A C T I C E
South Pasadena AP Chemistry Name 2 Chemical Kinetics Period Date U N I T T E S T P R A C T I C E Part 1 Multiple Choice You should allocate 30 minutes to finish this portion of the test. No calculator
More informationEXPERIMENT 23 Lab Report Guidelines
EXPERIMENT 23 Listed below are some guidelines for completing the lab report for Experiment 23: For each part, follow the procedure outlined in the lab manual. Observe all safety rules, including wearing
More informationEXPERIMENT A4: PRECIPITATION REACTION AND THE LIMITING REAGENT. Learning Outcomes. Introduction
1 EXPERIMENT A4: PRECIPITATION REACTION AND THE LIMITING REAGENT Learning Outcomes Upon completion of this lab, the student will be able to: 1) Demonstrate the formation of a precipitate in a chemical
More informationThe Mole. Relative Atomic Mass Ar
STOICHIOMETRY The Mole Relative Atomic Mass Ar Relative Molecular Mass Mr Defined as mass of one atom of the element when compared with 1/12 of an atom of carbon-12 Some Ar values are not whole numbers
More informationLecture (8) Effect of Changing Conditions on the Rate Constant
Lecture (8) Effect of Changing Conditions on the Rate Constant The relationship between the rate of a chemical reaction and the concentration of the reactants is shown by the rate equation of the reaction.
More informationEXPERIMENT - 2 DETERMINE THE PRODUCT OF A REDOX REACTION REACTION OF BROMATE AND HYDROXYLAMMONIUM IONS CHM110H5F
EXPERIMENT - 2 DETERMINE THE PRODUCT OF A REDOX REACTION REACTION OF BROMATE AND HYDROXYLAMMONIUM IONS CHM110H5F EXPERIMENT PERFORMED ON: 03 OCTOBER, 2012 REPORT SUBMITTED ON: 10 OCTOBER, 2012 SUBMITTED
More informationPreparation of a Coordination Compound. Step 1 Copy the balanced equation for the preparation of FeC 2 O 4.. 3H2 O from FeC 2 O 4. Mass of watch glass
Student Name Lab Partner Demonstrator Lab Section DATA SHEET Marking scheme Prelab exercise Lab performance Sig figs, units Calculations Crystals Preparation of a Coordination Compound Step 1 Copy the
More informationSolubility Product Constant (K sp ) and the Common-Ion Effect for Calcium Iodate, a Salt of Limited Solubility
Solubility Product Constant (K sp ) and the Common-Ion Effect for Calcium Iodate, a Salt of Limited Solubility Purpose Determine the solubility product constant (K sp ) for a sparingly soluble salt. Study
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 informationRATE LAW DETERMINATION OF CRYSTAL VIOLET HYDROXYLATION
Rate Law Determination of Crystal Violet Hydroxylation Revised 5/22/12 RATE LAW DETERMINATION OF CRYSTAL VIOLET HYDROXYLATION Adapted from "Chemistry with Computers" Vernier Software, Portland OR, 1997
More informationEXPERIMENT 22 SOLUBILITY OF A SLIGHTLY SOLUBLE ELECTROLYTE
EXPERIMENT 22 SOLUBILITY OF A SLIGHTLY SOLUBLE ELECTROLYTE INTRODUCTION Electrolytes are compounds that are present in solution as ions. They are more likely to be soluble in water than in most other liquids
More informationEXPERIMENT C3: SOLUBILITY PRODUCT & COMMON ION EFFECT. Learning Outcomes. Introduction. Upon completion of this lab, the student will be able to:
1 EXPERIMENT C3: SOLUBILITY PRODUCT & COMMON ION EFFECT Learning Outcomes Upon completion of this lab, the student will be able to: 1) Measure the solubility product constant for a sparingly soluble salt.
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 informationExperiment 2: Analysis of Commercial Bleach Solutions
Experiment 2: Analysis of Commercial Bleach Solutions I. Introduction The ability of household bleach to remove stains is related to the amount of oxidizing agent in it. The oxidizing agent in bleach is
More informationChapter: Chemical Kinetics
Chapter: Chemical Kinetics Rate of Chemical Reaction Question 1 Nitrogen pentaoxide decomposes according to equation: This first order reaction was allowed to proceed at 40 o C and the data below were
More informationThe Kinetics of the Iodine Clock Reaction
Experiment 2 Pre-lab Assignment Before coming to lab: Read the lab thoroughly. Answer the pre-lab questions that appear at the end of this lab exercise. The questions should be answered on a separate (new)
More informationDate Completed: Lab Partner(s):
Name: Lab Partner(s): Date Completed: Lab # 23: Factors Affecting Reaction Rate Accelerated Chemistry 1 Purpose Did you ever wonder why certain chemicals when mixed do not react; yet others upon immediate
More informationL = 6.02 x mol Determine the number of particles and the amount of substance (in moles)
1.1 The Mole 1.1.1 - Apply the mole concept to substances A mole is the name given to a certain quantity. It represents 6.02 x 10 23 particles. This number is also known as Avogadro's constant, symbolised
More informationClocking the Effect of Molarity on Speed of Reaction. reaction. While most people do assume that the temperature of the solution is often the most
Ding 1 Chunyang Ding Mr. Rierson AP/IB Chemistry SL 28 January 2013 Clocking the Effect of Molarity on Speed of Reaction In basic levels of chemistry, most of the experimenter s attention is on the reaction
More informationThere is not enough activation energy for the reaction to occur. (Bonds are pretty stable already!)
Study Guide Chemical Kinetics (Chapter 12) AP Chemistry 4 points DUE AT QUIZ (Wednesday., 2/14/18) Topics to be covered on the quiz: chemical kinetics reaction rate instantaneous rate average rate initial
More informationRight Side NOTES ONLY
Ch. 8 Stoichiometry Title and Highlight TN Ch 8.1 Topic: EQ: Right Side NOTES ONLY Date Write Question out (left side of red line) and answer it (Highlight answer) based on from what you read. Write out
More informationRate law: rate = - [ ]/ t = k [ ] x where x = order. Rate constant = k depends on T (k = Ae -Ea/RT )
Chem 1B Objective 5: Understand factors that determine reaction rate and describe reaction rate with rate law, order, rate constant, and activation energy. Key Ideas: Important in preserving food, curing
More informationCHEM 116 Collision Theory and Reaction Mechanisms
CHEM 116 Collision Theory and Reaction Mechanisms Lecture 13 Prof. Sevian Note: If there is anything we do not finish about reaction mechanisms today, that is where we will start on Tuesday with Lecture
More informationThe rate of reaction is defined as the change in concentration of a substance in unit time Its usual unit is mol dm -3 s -1
5.1.1 ow Fast? The rate of reaction is defined as the change in concentration of a substance in unit time Its usual unit is mol dm -3 s -1 When a graph of concentration of reactant is plotted vs time,
More informationTECHNICAL SCIENCE DAS12703 ROZAINITA BT. ROSLEY PUSAT PENGAJIAN DIPLOMA UNVERSITI TUN HUSSEIN ONN MALAYSIA
TECHNICAL SCIENCE DAS12703 ROZAINITA BT. ROSLEY PUSAT PENGAJIAN DIPLOMA UNVERSITI TUN HUSSEIN ONN MALAYSIA ii TABLE OF CONTENTS TABLE OF CONTENTS... i LIST OF FIGURES... iii Chapter 1... 4 SOLUTIONS...
More informationALE 1. Chemical Kinetics: Rates of Chemical Reactions
Name Chem 163 Section: Team Number: ALE 1. Chemical Kinetics: Rates of Chemical Reactions (Reference: Sections 16.1 16.2 + parts of 16.5 16.6 Silberberg 5 th edition) How do the surface area, concentration
More information5. What is the name of the phase transition that occurs when a solid is converted directly into a gas (without going through the liquid phase)?
1. If the volume of a confined gas is doubled while the temperature remains constant, what change (if any) would be observed in the pressure? a. It would be half as large. b. It would double. c. It would
More informationLIMITING REAGENT. Taking Stoichiometric conversions one step further
LIMITING REAGENT Taking Stoichiometric conversions one step further Limiting Reagent The reactant that limits the amount of product that can be formed. The reaction will stop when all of the limiting reactant
More information1. KINETICS. Kinetics answers
1. KINETICS 1.1. Rate determining step 1.2. Calculating reaction rate 1.3. Measuring reaction rate in the lab 1.4. Determining the rate equation 1.5. Arrhenius and rate Kinetics answers 1.1. Rate determining
More informationSafety Note: Safety glasses and laboratory coats are required when performing this experiment
The Determination of Hypochlorite in Bleach Reading assignment: Burdge, Chemistry 4 th edition, section 4.6. We will study an example of a redox titration in order to determine the concentration of sodium
More informationTitration of HCl with Sodium Hydroxide
Titration of HCl with Sodium Hydroxide Lab Report for the Subject of Advanced Chemistry Anon Durongpisitkul, Karis Katekovit, Varun Saketharam,Thanon Thamvorapol, Chanon Anektanasup- January 28, 2017 1
More informationUnit - 4 CHEMICAL KINETICS VSA QUESTIONS (1 - MARK QUESTIONS) (aq) as product for the reaction : 5 Br (aq) + Br(aq) + 6H + (aq) 3 Br 2
Unit - 4 CHEMICAL KINETICS VSA QUESTIONS (1 - MARK QUESTIONS) 1. Define the term rate of reaction. 2. Mention the units of rate of reaction. 3. Express the rate of reaction in terms of Br (aq) as reactant
More informationFactors That Affect Rates. Factors That Affect Rates. Factors That Affect Rates. Factors That Affect Rates
KINETICS Kinetics Study of the speed or rate of a reaction under various conditions Thermodynamically favorable reactions DO NOT mean fast reactions Some reactions take fraction of a second (explosion)
More informationIntroductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed.
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University of Illinois Chapter 9 Chemical Quantities Information
More information1. An aqueous solution of calcium bromide has a concentration of molal. The percent by mass of calcium bromide in the solution is:
1. An aqueous solution of calcium bromide has a concentration of 0.441 molal. The percent by mass of calcium bromide in the solution is: a. 5.00% b. 8.10% c. 10.10% d. 12.15% e. 16.20% 2. The melting point
More informationChemistry 201: General Chemistry II - Lecture
Chemistry 20: General Chemistry II - Lecture Dr. Namphol Sinkaset Chapter 5 Study Guide Concepts. rate of reaction: the speed at which reactants disappear and products form. 2. There can only be one numerical
More information15.0 g Fe O 2 mol Fe 55.8 g mol Fe = g
CHAPTER Practice Questions.1 1 Mg, O, H and Cl (on each side).. BaCl (aq) + Al (SO ) (aq) BaSO (s) + AlCl (aq).5 0.15 mol 106 g mol 1 = 1. g 15.0 g Fe O mol Fe 55.8 g mol Fe = 10.9 g 1 159.7 g mol FeO
More informationDETERMINATION OF K c FOR AN EQUILIBRIUM SYSTEM
DETERMINATION OF K c FOR AN EQUILIBRIUM SYSTEM 1 Purpose: To determine the equilibrium constant K c for an equilibrium system using spectrophotometry to measure the concentration of a colored complex ion.
More informationDetermination of the Rate Constant for an Iodine Clock Reaction
CHEM 122L General Chemistry Laboratory Revision 1.3 Determination of the Rate Constant for an Iodine Clock Reaction To learn about Integrated Rate Laws. To learn how to measure a Rate Constant. To learn
More informationTitrations Worksheet and Lab
Titrations Worksheet and Lab Vocabulary 1. Buret: a piece of glassware used for dispensing accurate volumes, generally reads to two places of decimal. 2. Titrant: the substance of known concentration added
More informationRates and Temperature
Rates and Temperature N Goalby Chemrevise.org Activation Energy Molecules will only react if they collide with enough energy to break the relevant bonds in one or either of the reactant molecules. This
More informationPartner: Judy 29 March Analysis of a Commercial Bleach
Partner: Judy 29 March 2012 Analysis of a Commercial Bleach Purpose: The purpose of this lab is to determine the amount of sodium hypochlorite (NaClO) in commercial bleach. This can be done by forming
More informationExperiment 7 Buffer Capacity & Buffer Preparation
Chem 1B Dr. White 57 Experiment 7 Buffer Capacity & Buffer Preparation Objectives To learn how to choose a suitable conjugate acid- base pair for making a buffer of a given ph To gain experience in using
More informationb. Free energy changes provide a good indication of which reactions are favorable and fast, as well as those that are unfavorable and slow.
Chem 130 Name Exam 3, Ch 7, 19, 14 November 9, 2018 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct
More information