Unit #10. Chemical Kinetics
|
|
- Darleen McDaniel
- 5 years ago
- Views:
Transcription
1 Unit #10 Chemical Kinetics Zumdahl Chapter 12 College Board Performance Objectives: Express the rate of a reaction in terms of changes in the concentration of a reactant or a product per time. Understand how to change from one to the other. Understand the difference graphically between average rate and instantaneous rate. Be able to calculate both. Explain the meaning of the reaction rate law and the rate law constant. Be able to determine a reaction rate law for a reaction from experimental data. Calculate the rate law constant (including units) after finding the rate law constant from experimental data. After this, calculate the rate of another experiment not included in the data. Understand what is meant by order in terms of a reactant as well as the overall order. Explain graphically the concept of activation energy and how temperature affects reaction rate. Understand how temperature affects the rate law constant for a reaction. Be able to relate the collision model to all of the above. Explain what is meant by a reaction mechanism and know the meaning of elementary steps, rate-determining step, and intermediate species. Be able to explain and show how a rate law is derived from a certain reaction mechanism. Describe the theory of how a catalyst works.
2 I. Reaction Rates A. Chemical Kinetics The Rate of a Chemical Reaction depends on 4 things: B. Reaction Rate 1. Average Rate = [reactant] or [product] t t 2. Instantaneous Rate 3. Sample Exercise Using the following data, calculate the average rate of disappearance of C 4 H 9 Cl over the time interval from 50.0 to s C 4 H 9 Cl (l) + H 2 0 (l) C 4 H 9 OH (aq) + HCl (aq) Time (s) [C 4 H 9 Cl] (M) C. Reaction Rates and Stoichiometry aa + bb cc + dd Rate = 1 [A] = 1 [B] = 1 [C] = 1 [D] a t b t c t d t 2
3 D. Sample Exercise 14.2 (a) How is the rate of disappearance of ozone related to the rate of appearance of oxygen in the following equation: 2 O 3 (g) 3 O 2 (g)? (b) If the rate of appearance of O 2 is 6.0 x 10 5 M/s at a particular instant, what is the value of the rate of disappearance of O 3 at this same time? II. The dependance of rate of concentration A. Rate Law An equation (expression) that relates the reaction rate to the [conc] of reactants (or sometimes products). Reaction Constant k a constant of proportionality between the reaction rate and [conc] of reactants that appear in the rate law. General Form = Rate = k[a] x [B] y [C] z. B. Reaction orders and Overall Reaction Order The exponents in the rate law expression (x,y,z) are called the rate order for those reactants. The sum of all the rate orders in the rate law expression is called the overall reaction order. Reaction orders are determined experimentally, not by the coefficients from the balanced chemical equation. C. Units of Rate Constants Units of rate constants are important in helping to solve rate order problems Units of Rate = (Units of Rate Constant) (Units of Concentration) x D. Sample Exercise 14-3 (a) What are the overall reaction orders for the following reactions? #1 2N 2 O 5 (g) 4NO 2 (g) + O 2 (g) Rate = k[n 2 O 5 ] #2 CHCl 3 (g) + Cl 2 (g) CCl 4 (g) + HCl Rate = k[chcl 3 ] [Cl 2 ] 1/2 (b) What are the usual units of the rate constant for the rate law for equation #1? 3
4 E. Using Initial Rates to Determine Rate Laws Consider the reaction below between bromate and bromide ions in acid solution. The reactions kinetics can be studied and some results are given in the table. BrO 3 -(aq) + 5Br - (aq) + 6H + (aq) 3Br 2(aq) + 3H 2 O (l) Initial concentrations Mixture [BrO - 3 ] / M [Br - ] / M [H + ] / M Relative Rate A B C D By comparing the results from mixtures A & B; Doubling [BrO 3 - ] doubles the rate. (Note the other concentrations are kept constant to ensure a fair test). Therefore the rate α [BrO 3 - ] and the rate is said to be first order with respect to, (w.r.t), [BrO 3 - ]. By comparing the results from mixtures B & C; Doubling the [Br - ] doubles the rate. (Note the other concentrations are kept constant to ensure a fair test). Therefore the rate α [Br - ] and the rate is said to be first order w.r.t [Br - ]. By comparing the results from mixtures C & D; Doubling the [H + ] quadruples the rate. (Note the other concentrations are kept constant to ensure a fair test). Therefore the rate α [H + ] 2 and the rate is said to be second order w.r.t [H + ]. Combining these results gives Rate [BrO 3 - ][Br - ][H + ] 2 And introducing the rate constant (k), the equation becomes Rate = k[bro 3 - ][Br - ][H + ] 2 F. Sample Exercise 14.4 The initial rate of a reaction A + B C was measured for several different starting concentrations of A and B, with the results given below: Experiment # [A] (M) [B] (M) Initial Rate (M/s) x x x 10 5 Determine (a) the rate law for the reaction; (b) the magnitude of the rate constant; (c) the rate of the reaction when [A] = M and [B] = M. 4
5 III. Change of Concentration with Time A. First Order Reactions Rxn whose rate depends on the [conc] of a single reactant (raised to the first power) Rate = [A] = k [A] ln[a] t - ln[a] 0 = - k t t ln[a] 0 = - k t + ln[a] t y = m x + b B. Half Life - t 1/2 - the time required for the reactant concentration to drop to one half of its initial value. For a 1 st Order Rxn t 1/2 = k C. Second Order Reactions Rate depends on the reactant concentration raised to the second power. For Rate = k [A] 2 1 = k t + 1 [A] t [A] 0 D. Sample Exercises 14.5 The first-order rate constant for the decomposition of a certain insecticide in water at 12 C is 1.45 yr 1, A quantity of this insecticide is washed into a lake in June, leading to a [ ] of 5.0 x 10 7 g/cm 3 of water. Assume that the effective temperature of the lake is 12 C, (a) What is the concentration of the insecticide in June of the following year? (b) How long will it take for the concentration of the insecticide to drop to 3.0 x 10 7 g/cm 3? 14.7 The following data were obtained for the gas-phase decomposition of nitrogen dioxide at 300 C, 2NO 2 (g) 2 NO(g) + O 2 (g) Is the reaction 1 st or 2 nd Order? Time (s) [NO 2 ] (M) Time (s) [NO 2 ] (M)
6 IV. Temperature and Rate A. The Collision Model As a guideline in many reactions a 10 o C rise will result in an approximate doubling of the rate. Consider the Maxwell- Boltzman distribution graph of molecular energies. The area underneath the graph represents the total number of molecules. At higher temperatures, (T high), the average energy of the molecules is greater and a greater number of molecules will have energies > E a. (i.e. the area to the right of Eact underneath the T high curve in the graph above is much larger than that of the area to the right of Eact underneath the T low curve). A reaction will always be much faster at a higher temperature because many more molecules possess the activation energy on collision. In addition, as the temperature increase so will the number of collisions. 6
7 B. Activation Energy (i) The activation energy is always endothermic regardless of the overall heat change. (ii) H is positive for an endothermic reaction and negative for an exothermic reaction. (iii) The maximum energy state (TS) is called the transition state or activated complex and can be regarded as the point at which the bonds in the reactants have (or are about to be) broken and the bonds in the products have (or are about to be) formed. (iv) A comparison of (Y) and (Z) shows that H is the same in each reaction. It shows that the products in both reactions are thermodynamically more stable (and to the same extent) than the reactants. (Y) however has a lower activation energy meaning that the reactants in this reaction are less kinetically stable than those in (Z). i.e. the reaction in (Y) will proceed at a faster rate. C. The Arrhenius Equation V. Reaction Mechanisms A. Elementary Steps B. Intermediate Steps 7
8 C. Rate Laws of Elementary Processes D. Rate Laws of Multistep Mechanism 1. Rate-determining Step 2. Mechanism with an initial fast step 8
9 VI. Catalyst A. Definition A. Homogeneous Catalyst B. Heterogeneous Catalyst C. Enzymes 9
10 1. For each table of data below, deduce the orders of reaction, the rate equation, the rate constant and the units of the rate constant. Experiment Starting [A] / M Starting [T] / M Rate / Ms Experiment Starting [C] / M Starting [D] / M Rate / Mhr Experiment Starting [X] / M Starting [Y] / M Rate / Mmin The table below shows the results of an investigation into the rate of reaction between hydroxide ions and phosphinate ions (PH 2 O 2 - ) at 80 o C. Experiment [phosphinate ion] / moldm -3 [hydroxide ion] / moldm -3 Rate / cm3 min (i) (ii) What is the rate expression for this reaction? Calculate the rate constant k, and give its units. 10
11 D. Summary of graphical interpretations of orders of reaction Order Zero First Second Rate Law Rate = k Rate = k [A] Rate = k [A] 2 Integrated rate law [A] = -kt + [A] 0 ln [A] = -kt + ln [A] 0 Plot to give straight line [A] versus t ln [A] versus t versus t Slope (gradient) Slope = -k Slope = -k Slope =k Half-life 11
Kinetics - Chapter 14. reactions are reactions that will happen - but we can t tell how fast. - the steps by which a reaction takes place.
The study of. Kinetics - Chapter 14 reactions are reactions that will happen - but we can t tell how fast. - the steps by which a reaction takes place. Factors that Affect Rx Rates 1. The more readily
More informationChapter 14. Chemical Kinetics
Chapter 14. Chemical Kinetics Common Student Misconceptions It is possible for mathematics to get in the way of some students understanding of the chemistry of this chapter. Students often assume that
More informationBrown et al, Chemistry, 2nd ed (AUS), Ch. 12:
Kinetics: Contents Brown et al, Chemistry, 2 nd ed (AUS), Ch. 12: Why kinetics? What is kinetics? Factors that Affect Reaction Rates Reaction Rates Concentration and Reaction Rate The Change of Concentration
More information14.1 Factors That Affect Reaction Rates
14.1 Factors That Affect Reaction Rates 1) 2) 3) 4) 14.2 Reaction Rates How does increasing the partial pressures of the reactive components of a gaseous mixture affect the rate at which the compounds
More informationChemical. Chapter 14. Kinetics. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E.
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 14 1 PDF Created with deskpdf PDF www.farq.xyz Writer - Trial :: http://www.docudesk.com
More informationHow fast reactants turn into products. Usually measured in Molarity per second units. Kinetics
How fast reactants turn into products. Usually measured in Molarity per second units. Kinetics Reaction rated are fractions of a second for fireworks to explode. Reaction Rates takes years for a metal
More informationKinetics. Chapter 14. Chemical Kinetics
Lecture Presentation Chapter 14 Yonsei University In kinetics we study the rate at which a chemical process occurs. Besides information about the speed at which reactions occur, kinetics also sheds light
More informationChapter 14 Chemical Kinetics
Chapter 14 14.1 Factors that Affect Reaction Rates 14.2 Reaction Rates 14.3 Concentration and Rate Laws 14.4 The Change of Concentration with Time 14.5 Temperature and Rate 14.6 Reaction Mechanisms 14.7
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 informationLecture Presentation. Chapter 14. Chemical Kinetics. John D. Bookstaver St. Charles Community College Cottleville, MO Pearson Education, Inc.
Lecture Presentation Chapter 14 John D. Bookstaver St. Charles Community College Cottleville, MO In kinetics we study the rate at which a chemical process occurs. Besides information about the speed at
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 informationChemical Kinetics. Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of reactions:
Chemical Kinetics Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of reactions: reactant concentration temperature action of catalysts surface
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 informationChapter 14. Chemical Kinetics
Sample Exercise 14.1 (p. 578) For the reaction pictured at the bottom of the previous page, calculate the average rate at which A disappears over the time interval from 20 s to 40 s. (1.2 x 10-2 M/s) Practice
More informationChapter 14 Chemical Kinetics
Chapter 14 Chemical Kinetics Learning goals and key skills: Understand the factors that affect the rate of chemical reactions Determine the rate of reaction given time and concentration Relate the rate
More informationChapter 14. Chemical Kinetics
14.1 Factors that Affect Reaction Rates Chemical kinetics = the study of how fast chemical reactions occur. Factors which affect rates of reactions: Physical state of the reactants. Concentration of the
More informationChemical Kinetics and Equilibrium
Chemical Kinetics and Equilibrium Part 1: Kinetics David A. Katz Department of Chemistry Pima Community College Tucson, AZ USA Chemical Kinetics The study of the rates of chemical reactions and how they
More informationChapter 12. Kinetics. Factors That Affect Reaction Rates. Factors That Affect Reaction Rates. Chemical. Kinetics
PowerPoint to accompany Kinetics Chapter 12 Chemical Kinetics Studies the rate at which a chemical process occurs. Besides information about the speed at which reactions occur, kinetics also sheds light
More informationChapter 13 Rates of Reactions
Chapter 13 Rates of Reactions Chemical reactions require varying lengths of time for completion, depending on the characteristics of the reactants and products. The study of the rate, or speed, of a reaction
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 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 informationCHEMISTRY. Chapter 14 Chemical Kinetics
CHEMISTRY The Central Science 8 th Edition Chapter 14 Kozet YAPSAKLI kinetics is the study of how rapidly chemical reactions occur. rate at which a chemical process occurs. Reaction rates depends on The
More informationCalculating Rates of Substances. Rates of Substances. Ch. 12: Kinetics 12/14/2017. Creative Commons License
Ch. 2: Kinetics An agama lizard basks in the sun. As its body warms, the chemical reactions of its metabolism speed up. Chemistry: OpenStax Creative Commons License Images and tables in this file have
More informationChemical Kinetics AP Chemistry Lecture Outline
Chemical Kinetics AP Chemistry Lecture Outline Name: Factors that govern rates of reactions. Generally... (1)...as the concentration of reactants increases, rate (2)...as temperature increases, rate (3)...with
More informationChemical 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 informationChapter 14. Chemical Kinetics
Common Student Misconceptions It is possible for mathematics to get in the way of some students understanding of the chemistry of this chapter. Students often assume that reaction orders may be determined
More informationC H E M I C N E S C I
C H E M I C A L K I N E T S C I 4. Chemical Kinetics Introduction Average and instantaneous Rate of a reaction Express the rate of a reaction in terms of change in concentration Elementary and Complex
More informationName AP CHEM / / Chapter 12 Outline Chemical Kinetics
Name AP CHEM / / Chapter 12 Outline Chemical Kinetics The area of chemistry that deals with the rate at which reactions occur is called chemical kinetics. One of the goals of chemical kinetics is to understand
More informationAP Chem Chapter 14 Study Questions
Class: Date: AP Chem Chapter 14 Study Questions 1. A burning splint will burn more vigorously in pure oxygen than in air because a. oxygen is a reactant in combustion and concentration of oxygen is higher
More informationLecture (3) 1. Reaction Rates. 2 NO 2 (g) 2 NO(g) + O 2 (g) Summary:
Summary: Lecture (3) The expressions of rate of reaction and types of rates; Stoichiometric relationships between the rates of appearance or disappearance of components in a given reaction; Determination
More informationChapter 13 Kinetics: Rates and Mechanisms of Chemical Reactions
Chapter 13 Kinetics: Rates and Mechanisms of Chemical Reactions 14.1 Focusing on Reaction Rate 14.2 Expressing the Reaction Rate 14.3 The Rate Law and Its Components 14.4 Integrated Rate Laws: Concentration
More informationReaction Rate. Rate = Conc. of A at t 2 -Conc. of A at t 1. t 2 -t 1. Rate = Δ[A] Δt
Kinetics The study of reaction rates. Spontaneous reactions are reactions that will happen - but we can t tell how fast. Diamond will spontaneously turn to graphite eventually. Reaction mechanism- the
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 informationOutline: Kinetics. Reaction Rates. Rate Laws. Integrated Rate Laws. Half-life. Arrhenius Equation How rate constant changes with T.
Chemical Kinetics Kinetics Studies the rate at which a chemical process occurs. Besides information about the speed at which reactions occur, kinetics also sheds light on the reaction mechanism (exactly
More informationExamples of fast and slow reactions
1 of 10 After completing this chapter, you should, at a minimum, be able to do the following. This information can be found in my lecture notes for this and other chapters and also in your text. Correctly
More informationChapter 14 Chemical Kinetics
Chapter 14 Chemical Kinetics Thermodynamics tells us what can happen and how far towards completion a reaction will proceed. Kinetics tells us how fast the reaction will go. Study of rates of reactions
More informationChapter 14. Chemical Kinetics
Chapter 14. Chemical Kinetics 14.1 Factors that Affect Reaction Rates The speed at which a chemical reaction occurs is the reaction rate. Chemical kinetics is the study of how fast chemical reactions occur.
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 informationChapter 14, Chemical Kinetics
Last wee we covered the following material: Review Vapor Pressure with two volatile components Chapter 14, Chemical Kinetics (continued) Quizzes next wee will be on Chap 14 through section 14.5. 13.6 Colloids
More informationAP CHEMISTRY CHAPTER 12 KINETICS
AP CHEMISTRY CHAPTER 12 KINETICS Thermodynamics tells us if a reaction can occur. Kinetics tells us how quickly the reaction occurs. Some reactions that are thermodynamically feasible are kinetically so
More informationChapter 14. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 14 John D. Bookstaver St. Charles Community College St. Peters, MO 2006, Prentice Hall,
More informationAP CHEMISTRY NOTES 7-1 KINETICS AND RATE LAW AN INTRODUCTION
AP CHEMISTRY NOTES 7-1 KINETICS AND RATE LAW AN INTRODUCTION CHEMICAL KINETICS the study of rates of chemical reactions and the mechanisms by which they occur FACTORS WHICH AFFECT REACTION RATES 1. Nature
More informationChapter 14: Chemical Kinetics
Chapter 14: Chemical Kinetics NOTE THIS CHAPTER IS #2 TOP TOPICS ON AP EXAM!!! NOT ONLY DO YOU NEED TO FOCUS ON THEORY (and lots of MATH) BUT YOU MUST READ THE FIGURES TOO!!! Ch 14.1 ~ Factors that Affect
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 informationChapter 30. Chemical Kinetics. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved.
Chapter 30 Chemical Kinetics 1 Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved. Chemists have three fundamental questions in mind when they study chemical reactions: 1.) What happens?
More informationChemical Kinetics -- Chapter 14
Chemical Kinetics -- Chapter 14 1. Factors that Affect Reaction Rate (a) Nature of the reactants: molecular structure, bond polarity, physical state, etc. heterogeneous reaction: homogeneous reaction:
More informationChapter 14 Chemical Kinetics
How fast do chemical processes occur? There is an enormous range of time scales. Chapter 14 Chemical Kinetics Kinetics also sheds light on the reaction mechanism (exactly how the reaction occurs). Why
More informationAP Chapter 13: Kinetics Name
AP Chapter 13: Kinetics Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 13: Kinetics 2 Warm-Ups (Show your work for credit) Date 1.
More informationChapter 12. Chemical Kinetics
Chapter 12 Chemical Kinetics Section 12.1 Reaction Rates Reaction Rate Change in concentration of a reactant or product per unit time. Rate = concentration of A at time t t 2 1 2 1 concentration of A at
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 EXERCISE 14.3 Relating Rates at Which Products Appear and Reactants Disappear
SAMPLE EXERCISE 14.3 Relating Rates at Which Products Appear and Reactants Disappear (a) How is the rate at which ozone disappears related to the rate at which oxygen appears in the reaction (b) If the
More informationChapter 14. Chemical Kinetics
Chapter 14. Chemical Kinetics Common Student Misconceptions It is possible for mathematics to get in the way of some students understanding of the chemistry of this chapter. Students often assume that
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 informationLecture Presentation. Chapter 14. James F. Kirby Quinnipiac University Hamden, CT. Chemical Kinetics Pearson Education, Inc.
Lecture Presentation Chapter 14 James F. Kirby Quinnipiac University Hamden, CT In chemical kinetics we study the rate (or speed) at which a chemical process occurs. Besides information about the speed
More information14.1 Expressing the Reaction Rate
14.1 Expressing the Reaction Rate Differential Rate and Integrated Rate Laws Fred Omega Garces Chemistry 201 Miramar College 1 Expressing Reaction Rates Outline Kinetics: Intro Factors influencing Reaction
More informationKinetics CHAPTER IN THIS CHAPTER
CHAPTER 14 Kinetics IN THIS CHAPTER Summary: Thermodynamics often can be used to predict whether a reaction will occur spontaneously, but it gives very little information about the speed at which a reaction
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 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 informationWhat we learn from Chap. 15
Chemical Kinetics Chapter 15 What we learn from Chap. 15 15. The focus of this chapter is the rates and mechanisms of chemical reactions. The applications center around pesticides, beginning with the opening
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 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 information2/23/2018. Familiar Kinetics. ...and the not so familiar. Chemical kinetics is the study of how fast reactions take place.
CHEMICAL KINETICS & REACTION MECHANISMS Readings, Examples & Problems Petrucci, et al., th ed. Chapter 20 Petrucci, et al., 0 th ed. Chapter 4 Familiar Kinetics...and the not so familiar Reaction Rates
More informationChemistry 102 Chapter 14 CHEMICAL KINETICS. The study of the Rates of Chemical Reactions: how fast do chemical reactions proceed to form products
CHEMICAL KINETICS Chemical Kinetics: The study of the Rates of Chemical Reactions: how fast do chemical reactions proceed to form products The study of Reaction Mechanisms: the steps involved in the change
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 informationChemical Kinetics. What Influences Kinetics?
Chemical Kinetics Predictions of likelihood for a reaction to occur have been based on difference in energy between products and reactants: Thermodynamics only compares reactants to products, says nothing
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 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 informationRates of Chemical Reactions
Rates of Chemical Reactions Jim Birk 12-1 Questions for Consideration 1. What conditions affect reaction rates? 2. How do molecular collisions explain chemical reactions? 3. How do concentration, temperature,
More informationChapter 16. Rate Laws. The rate law describes the way in which reactant concentration affects reaction rate.
Rate Laws The rate law describes the way in which reactant concentration affects reaction rate. A rate law is the expression that shows how the rate of formation of product depends on the concentration
More informationChapter 12 - Chemical Kinetics
Chapter 1 - Chemical Kinetics 1.1 Reaction Rates A. Chemical kinetics 1. Study of the speed with which reactants are converted to products B. Reaction Rate 1. The change in concentration of a reactant
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 informationReaction Rate. Products form rapidly. Products form over a long period of time. Precipitation reaction or explosion
Reaction Rate Products form rapidly Precipitation reaction or explosion Products form over a long period of time Corrosion or decay of organic material Chemical Kinetics Study of the rate at which a reaction
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 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 Chapter 14. Chemical Kinetics (Homework) Ky40
CHEM 1412. Chapter 14. Chemical Kinetics (Homework) Ky40 1. Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2ClO 2 (aq) + 2OH (aq) ClO
More informationCHAPTER 10 CHEMICAL KINETICS
CHAPTER 10 CHEMICAL KINETICS Introduction To this point in our study of chemistry, we have been concerned only with the composition of the equilibrium mixture, not the length of time required to obtain
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 informationSuggested Answers to Chemical Kinetics Revision Exercise. The results of some investigations of the rate of this reaction are shown below.
Suggested Answers to Chemical Kinetics Revision Exercise 1 At 973K, nitrogen monoxide and hydrogen react as follows: 2NO(g) + 2H 2 (g) N 2 (g) + 2H 2 O(g) The results of some investigations of the rate
More informationKinetics. 1. Consider the following reaction: 3 A 2 B How is the average rate of appearance of B related to the average rate of disappearance of A?
Kinetics 1. Consider the following reaction: 3 A 2 B How is the average rate of appearance of B related to the average rate of disappearance of A? A. [A]/ t = [B]/ t B. [A]/ t = (2/3)( [B]/ t) C. [A]/
More informationPart One: Reaction Rates. 1. Rates of chemical reactions. (how fast products are formed and/or reactants are used up)
A. Chemical Kinetics deals with: CHAPTER 13: RATES OF REACTION Part One: Reaction Rates 1. Rates of chemical reactions. (how fast products are formed and/or reactants are used up) 2. Mechanisms of chemical
More informationUnit 12: Chemical Kinetics
Unit 12: Chemical Kinetics Author: S. Michalek Introductory Resources: Zumdahl v. 5 Chapter 12 Main Ideas: Integrated rate laws Half life reactions Reaction Mechanisms Model for chemical kinetics Catalysis
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 informationCh part 2.notebook. November 30, Ch 12 Kinetics Notes part 2
Ch 12 Kinetics Notes part 2 IV. The Effect of Temperature on Reaction Rate Revisited A. According to the kinetic molecular theory of gases, the average kinetic energy of a collection of gas molecules is
More informationChapter 14 Chemical Kinetics
7/10/003 Chapter 14 Chemical Kinetics 14-1 Rates of Chemical Reactions 14- Reaction Rates and Concentrations 14-3 The Dependence of Concentrations on Time 14-4 Reaction Mechanisms 14-5 Reaction Mechanism
More informationGeneral Chemistry I Concepts
Chemical Kinetics Chemical Kinetics The Rate of a Reaction (14.1) The Rate Law (14.2) Relation Between Reactant Concentration and Time (14.3) Activation Energy and Temperature Dependence of Rate Constants
More informationYes. Yes. Yes. Experimental data: the concentration of a reactant or product measured as a function of time. Graph of conc. vs.
Experimental data: the concentration of a reactant or product measured as a function of time Graph of conc. vs. time Is graph a straigh t line? No Graph of ln[conc.] vs. time Yes System is zero order Is
More information11/9/2012 CHEMICAL REACTIONS. 1. Will the reaction occur? 2. How far will the reaction proceed? 3. How fast will the reaction occur?
CHEMICAL REACTIONS LECTURE 11: CHEMICAL KINETICS 1. Will the reaction occur? 2. How far will the reaction proceed? 3. How fast will the reaction occur? CHEMICAL REACTIONS C(s, diamond) C(s, graphite) G
More informationChapter 14: Chemical Kinetics
1. Which one of the following units would not be an acceptable way to express reaction rate? A) M/s B) M min 1 C) L mol 1 s 1 D) mol L 1 s 1 E) mmhg/min 3. For the reaction BrO 3 + 5Br + 6H + 3Br 2 + 3H
More informationthe following equilibrium constants. Label the thermodynamic and kinetic regions.
REACTION RATES 1. Distinguish between kinetic and thermodynamic regions of a reaction. 2. How does an increase in pressure affect the rate of a gas-phase reaction? What effect on the rate would doubling
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 information12.1 Reaction Rates. Reaction rate is defined as the change in concentration of a reactant or product per time. 2NO2 2NO + O2. In terms of reactants:
Kinetics Unit 5 12.1 Reaction Rates Reaction rate is defined as the change in concentration of a reactant or product per time. 2NO2 2NO + O2 In terms of reactants: The rate will be negative because the
More informationO 3 + UV photon (λ < 320 nm) O 2 * + O* O 3 + O 2O 2
Tro Chpt 13 Chemical Kinetics Rate of a chemical reaction Effect of concentration on reaction rate Integrated rate laws: How concentrations change with time Effect of temperature on rate Reaction mechanisms
More informationKinetics. Mary J. Bojan Chem Rate: change that occurs in a given interval of time.
Kinetics Rates of reaction average rates instantaneous rates Dependence of rate on concentration rate constant rate laws order of the reaction Dependence of rate on time First order Second order Half-life
More informationNAME: Chapter 14Chemical Kinetics (Reaction Rate Law Concepts)
NAME: Chapter 14Chemical Kinetics (Reaction Rate Law Concepts) 1. Go to the website : http://www.chm.davidson.edu/vce/kinetics/index.html, a. Go to reaction rates page, read the introductory paragraphs
More informationHomework #4 Chapter 15 Chemical Kinetics. Therefore, k depends only on temperature. The rate of the reaction depends on all of these items (a d).
Homework #4 Chapter 5 Chemical Kinetics 8. Arrhenius Equation Therefore, k depends only on temperature. The rate of the reaction depends on all of these items (a d). 4. a) d) b) c) e) 5. Rate has units
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 informationLecture 8, Kinetics 22/04/2018. Chemical kinetics studies: Rate. Kinetics, rate of the reaction, reaction mechanism. rates of chemical reactions
/04/08 Chemical kinetics studies: rates of chemical reactions the factors that affect rate reactions Lecture 8, Kinetics the mechanisms (the series of steps) by which reactions occur Rate We are all familiar
More information