!n[a] =!n[a] o. " kt. Half lives. Half Life of a First Order Reaction! Pressure of methyl isonitrile as a function of time!

Size: px
Start display at page:

Download "!n[a] =!n[a] o. " kt. Half lives. Half Life of a First Order Reaction! Pressure of methyl isonitrile as a function of time!"

Transcription

1 Half lives Half life: t 1/2 t 1/2 is the time it takes for the concentration of a reactant to drop to half of its initial value. For the reaction A! products Half Life of a First Order Reaction! Pressure of methyl isonitrile as a function of time! What is the half life according to the graph below?! 1.! 75 s! 2.! s! 3.! s! t 1/2 is where [A] = [A] o 2 For 1 st order reactions: What is t 1/2?!n[A] =!n[a] o " kt First order t 1/2 doesn t depend on concentration CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics 4-6 2

2 HALF LIFE OF 2 ND ORDER REACTIONS 1 A [ ] = k t + 1 A [ ] 0 To get t 1/2, we let [A] = 1/2 [A] o HALF LIFE OF A SECOND ORDER REACTION NO 2 (g)! NO(g) + 1/2 O 2 (g) [NO 2 ] M t 1/2 = Time (sec) t 1/2 of a Second Order Reaction depends on the initial concentration: [A] 0 CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics 4-6 4

3 Half Life Problem It requires 100 years for a first-order reaction to go 30.0% of the way to completion. What is the halflife of the reaction? Temperature Dependence of Reaction Rates CH 3 "N#C:! CH 3 " C # N: Rate = k [CH 3 "N#C:] Measure rate at different temperatures: Rates remain first order in [CH 3 "N#C:] What variable must change? CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics 4-6 6

4 Temperature Dependence of Reaction Rates For a reaction to occur; 1.!A molecular collision must occur 2.! The orientation of the molecules may determine the effectiveness of the collision. Temperature dependence of Reaction Rates As T increases what happens to reaction rate? Why? What about unimolecular reactions? Look at energy profile for a typical reaction: isonitrile isomerizes to form acetonitrile Cl + NOCl!! Cl 2 + NO! Cl + NOCl!! Cl + NOCl! CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics 4-6 8

5 Activation Energy %E= Temperature Dependence of Kinetic Energy Energy required to go from reactants to a transition state is Activation Energy Transition State or Activated Complex: How do molecules get the energy needed to get over the barrier? The fraction of molecules with a certain value of energy is f f $ e -Ea/RT What does increasing T do to f? CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics

6 Reaction Profiles For the reaction profiles below: 1.! What is %E? 2.! What is the activation energy? 3.! Which reaction will be fastest? Molecular level picture:!!reaction rate depends on frequency of collisions (& to concentration of reactants)!!reactants must come together with right orientation and enough KE to overcome E a How do orientation and activation energy factor into the rate laws? CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics

7 Arrhenius Equation k = A e E a RT ln k = ln A " E a RT! ARRHENIUS PLOT! ln k = ln A E a /RT How does this reaction happen? Does the C-N bond break? Find E a, compare to C-N Bond Energy of 293 kj/mole k = rate constant (temperature dependent) H 3 C N C! H 3 C C N A = frequency factor (Related to collision frequency and orientation) E a = Activation energy R = gas constant (usually J/mol-K) T = temperature in K Slope? Y Intercept? CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics

8 Compare k at different temperatures: eliminates A from the equation Understanding the high-temperature behavior of nitrogen oxides is essential for controlling pollution generated in automobile engines. 2NO(g)! N 2 (g)+ O 2 (g) The decomposition of nitric oxide (NO) to N 2 and O 2 is second order with a rate constant of M -1 s -1 at 737 C and M -1 s -1 at 947 C. Calculate the activation energy for the reaction. k ln k 2 = E R & 1 $ % T2 ' 1 a 1 T 1 #! " FYI Where does this equation come from? k ln k 2 = E R & 1 $ % T2 We want to eliminate A from the Arrhenius equation. This can be done if we know the reaction rate at two different temperatures: ln k 1 = " E a RT 1 ' 1 a 1 " ln A T 1 #! " ln k 2 = " E a RT 2 " ln A Subtracting eq 2 from equation one eliminates A ln k 1 " ln k 2 = " E a RT 1 ln k 1 k 2 = E a R # 1 " 1 & % ( $ T 2 T 1 ' # " "E & a % ( $ RT 2 ' R = J/mol-K CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics

9 How much does temperature affect rates? Most reactions have E a = kj/mol A typical E a might be 50 kj/mol How does rate vary over a 10 temperature range? (e.g. from 300 to 310 K) k ln k 2 = E & 1 R $ % T2 ' T 1 a 1 1 #! " REACTION MECHANISMS Reaction Mechanism: Process by which a reaction occurs; could be a multi-step reaction Start with elementary reactions: Process occurs in a single step. (Reaction proceeds as written with no other steps in between.) NO + O 3! NO 2 +O 2 k 2 /k 1 = e 0.65 = 1.9 (about twice as fast at 310 K compared to 300 K) For an elementary process Rate $ [reactants] Rate = k [NO][O 3 ] Rule of thumb: reaction rates double for every 10 rise in temperature (assumes E a ' 50 kj/mol) CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics

10 Reaction Mechanisms Most balanced reactions do not occur as a single elementary step. They occur as the net result of several elementary steps which could include such events as: "!Collisions "!Bonds Breaking "!Bonds Forming "!Groups of atoms changing orientation or relative position Elementary Reaction Molecularity: Unimolecular Bimolecular Termolecular This series of steps is called the REACTION MECHANISM CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics

11 Rates of Elementary Steps Reaction Rate A! B + C A + B! C + D For this reaction: NO 2 +CO! NO + CO 2 If rate obs = k[no 2 ][CO], is it an elementary process?! If rate obs " k[no 2 ][CO], is it an elementary process?! ( Propose a multistep mechanism: NO 2 + NO 2! NO 3 + NO step 1 NO 3 + CO! NO 2 + CO 2 step 2 NO 2 + CO! NO + CO 2 2A! C + D A + B + C! D + E CH112 LRSVDS Kinetics Possible Rate Laws for this multi-step mechanism: or [ ] rate = "# NO 2 #t [ ] #t "# CO rate = = k[ NO 2 ] 2 = k[ NO 3 ][ CO] Which is the rate law? Compare to experimental data to see which rate law matches. CH112 LRSVDS Kinetics

12 Experimental Data indicates: NO 2 +CO! NO + CO 2 Rate $ [NO 2 ] 2 It is possible to form Intermediates in a Mechanism NO 2 + NO 2! NO 3 + NO step 1 NO 3 + CO! NO 2 + CO 2 step 2 Which step of the mechanism is consistent with this data? NO 2 + CO! NO + CO 2 overall rxn Which step determines the rate of the entire reaction? The rate can t proceed any faster then the slowest step. SO: Rate Determining Step = Slow Step NO 3 is produced in step 1 and consumed in step 2. Note: an intermediate is NOT the same as an activated complex.!!intermediates do not appear in the rate law for the overall reaction.!!elementary steps must add up to eliminate intermediates and give the balanced equation for the overall process. CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics

13 To determine a mechanism for a reaction: 1.! Find the experimental rate law 2.! (Postulate elementary steps: this step will be done for you in Chem 112) 3.! Find the rate law predicted by the mechanism and compare it to the experimental data. "! No rate can be written in terms of intermediates If the first step is not rate determining, intermediates become involved in the rate law. Cl 2 + CHCl 3! HCl + CCl 4 Observed Rate = k obs [Cl 2 ] 1/2 [CHCl 3 ] Q: Is the following mechanism consistent with the experimental rate law? 1)! Cl 2 2Cl fast 2)! Cl + CHCl 3! HCl + CCl 3 slow 3)! Cl + CCl 3! CCl 4 fast CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics

14 Strategy for Determining Consistency of Proposed Mechanism Strategy: a) Overall reaction? b) Rate determining step? c)! Rate Law? d)! Define intermediate concentration in terms of reactants only In General: If a fast step comes before a slow step, solve for the concentration of an intermediate by assuming that the first step is an equilibrium. g)!substitute for intermediate in rate law h)!is it consistent? CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics

15 CATALYSIS Catalysis and Enzymes Read the supplemental reading on the class website: fall/handouts/supp_reading2.htm Definition of a Catalyst: How does it do this? Thermodynamic state functions are unaffected by catalysis (%E, % H, % G, % S ) (Why??) A Catalyst:!!!!!!!!!! CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics

16 Homogeneous catalysis: Catalyst is in the same phase as the reactants. Example: 2H 2 O 2 (l)! 2H 2 O(g) + O 2 (g) H H O O O O H H 2! H O O +! O H Heterogeneous catalysis: Catalyst is in a different phase than the reactants. H 2 + 1/2 O 2! H 2 O This reaction requires breaking strong H"H and O=O bonds ) ) 435 kj 498 kj (! Rate is negligible without a catalyst (!The stronger the bond, the more need for a catalyst to get a useful rate gas molecules H-H H-H O=O Pt surface solid adsorbed atoms H H O O diffusion on surface = = H O H H H O = CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics

17 Examples of Heterogeneous Catalysis Heterogeneous Catalysis in Nitrogen Fixation N 2 + 3H 2! 2NH 3 %G = K N#N triple bond (D = 946 kj) 1. Reaction of ethylene with hydrogen gas 2. Catalysis of Hydrogen Peroxide Decomposition by Manganese! Similar Mechanism! 3. Catalytic Converters! O 2 1) CO, C x H 2x+2! CO 2 (g) + H 2 O 2) NO, NO 2! N 2 (g) Catalysts: CuO, Cr 2 O 3, Pt, Pd, Rh CH112 LRSVDS Kinetics *!Microorganisms convert waste into N 2 (g), which must be turned into a form plants can use *!Plants accomplish this with the Enzyme. *!The best we can do is the Haber Process for Nitrogen Fixation CH112 LRSVDS Kinetics

18 Enzymes!! Biological catalysts.! Accelerate and control reaction rates.! Enormous protein molecules or combinations of proteins with other molecules.! Reactant is called a.! The region where substrates bind is called the. How Does Lowering E a AFFECT RATES? Uncatalyzed H 2 O 2! H 2 O + 1/2 O 2 Catalase (enzyme in liver) k cat k uncat = A cat e -E E a = 72 kj E a = 28 kj Compare k cat /k uncat at 37 C (body temp.) Assume A cat = A uncat (Is this a good assumption?) /RT a,cat A e -E a,uncat /RT uncat Catalase enzyme speeds up the decomposition rate by a factor of! Lysozyme CH112 LRSVDS Kinetics Peptidase enzymes break up proteins into amino acids (in your stomach). Similar effect on E a. CH112 LRSVDS Kinetics

19 Enzymes are superior to man-made catalysts 1.! More efficient ENZYME CATALYSIS Nature s catalysts how do they increase rates by > 10 10? Lock and Key Model: enzyme 2.! Absolute specificity binding sites k = A e -E /RT a reactant molecules enzyme-substrate complex 3.! Regulated 1.! Active site lowers E a how? products 2.! Enzyme-substrate complex stabilizes the transition state, activates the substrate 3.! Holds reactants in place ( high effective concentration (increases A) Each factor enhances rate by! 10 5 CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics

20 Enzyme Activity Depends on:! Temperature! ph! Concentration of substrate These conditions affect the active site by affecting the enzyme conformation ( ). (Left) Representation of an active site in an enzyme. Carbonic Anhydrase Enzyme Metal ions are often part of the active site and serve as the reaction center of the enzyme.! Zn 2+ ion at the active site! bound H 2 O displaced by CO 2! CO 2 activated & converted to HCO 3 - CO 2 + H 2 O! HCO H + (Right) Denatured enzyme parts of the active site are no longer in close proximity. CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics

21 VITAMINS!! Non-protein parts of enzymes, called co-enzymes.!! Combined with the protein they make an enzyme.!! Enzymes derived from vitamins play critical roles in redox chemistry in the body which is the source of heat and energy. Enzyme activity can be inhibited 1.! Denature Change shape via Temp. or ph change 2.! Competitive inhibition Bind a molecule to its active site, blocking any catalytic activity Many drugs and toxins work by this mechanism. Competitive inhibitors can be overcome by increasing the concentration of substrate. 3.! Non-competitive inhibition Bind a molecule to another site on enzyme: this results in a modification of the active site. 4. Irreversible Inhibitors Form strong covalent bonds to enzyme Increasing concentration of substrate has no effect. CH112 LRSVDS Kinetics CH112 LRSVDS Kinetics

22 DRUGS! Penicillin (antibiotic) blocks an enzyme that bacteria use to build cell walls.! People do not have this enzyme! Bacterial cells only are poisoned HIV-protease inhibitors bind to the active site of an enzyme that releases the viral coat proteins, preventing the production of the HIV virus. HIV protease Active site Ritonavir (inhibitor) CH112 LRSVDS Kinetics

Rate Law Summary. Rate Laws vary as a function of time

Rate Law Summary. Rate Laws vary as a function of time Rate Law Summary Measure the instantaneous rate of a reaction: this is a number with units of M/s! Measure the rate of loss of a reactant r... the rate of appearance of a product Repeat the experiment

More information

Chemical 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: 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 information

Reaction Mechanisms Dependence of rate on temperature Activation Energy E a Activated Complex Arrhenius Equation

Reaction Mechanisms Dependence of rate on temperature Activation Energy E a Activated Complex Arrhenius Equation Kinetics Dependence of rate on Concentration (RATE LAW) Reaction Mechanisms Dependence of rate on temperature Activation Energy E a Activated Complex Arrhenius Equation Mary J. Bojan Chem 112 1 A MECHANISM

More information

Kinetics. Chapter 14. Chemical Kinetics

Kinetics. 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 information

Chapter 14. Chemical Kinetics

Chapter 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

Chapter 14. Chemical Kinetics

Chapter 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 information

Chapter 14. Chemical Kinetics

Chapter 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 information

Chapter 14 Chemical Kinetics

Chapter 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 information

Chapter 14 Chemical Kinetics

Chapter 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 information

AP CHEMISTRY CHAPTER 12 KINETICS

AP 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 information

CHAPTER 12 CHEMICAL KINETICS

CHAPTER 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 information

Chapter 12. Chemical Kinetics

Chapter 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 information

Ch 13 Rates of Reaction (Chemical Kinetics)

Ch 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 information

Chapter 14. Chemical Kinetics

Chapter 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 information

Chapter 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 reaction orders may be determined

More information

Brown et al, Chemistry, 2nd ed (AUS), Ch. 12:

Brown 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 information

CHEM Chapter 14. Chemical Kinetics (Homework) Ky40

CHEM 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 information

Chemistry 102 Chapter 14 CHEMICAL KINETICS. The study of the Rates of Chemical Reactions: how fast do chemical reactions proceed to form products

Chemistry 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 information

Lecture 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. 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 information

Calculating Rates of Substances. Rates of Substances. Ch. 12: Kinetics 12/14/2017. Creative Commons License

Calculating 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 information

Chapter 14 Chemical Kinetics

Chapter 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 information

Chapter Chemical Kinetics

Chapter Chemical Kinetics CHM 51 Chapter 13.5-13.7 Chemical Kinetics Graphical Determination of the Rate Law for A Product Plots of [A] versus time, ln[a] versus time, and 1/[A] versus time allow determination of whether a reaction

More information

Chemical Kinetics AP Chemistry Lecture Outline

Chemical 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 information

Lecture (3) 1. Reaction Rates. 2 NO 2 (g) 2 NO(g) + O 2 (g) Summary:

Lecture (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 information

Chapter 12. Chemical Kinetics

Chapter 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 information

AP Chem Chapter 14 Study Questions

AP 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 information

Chapter 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 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 information

Chapter 14 Chemical Kinetics

Chapter 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 information

CHEMISTRY. Chapter 13. Chapter Outline. Factors Affecting Rate

CHEMISTRY. Chapter 13. Chapter Outline. Factors Affecting Rate CHEMISTRY Fifth Edition Gilbert Kirss Foster Bretz Davies Chapter 3 Chemical Kinetics: Reactions in the Atmosphere Chemistry, 5 th Edition Copyright 207, W. W. Norton & Company Chapter Outline 3.4 Reaction

More information

Chemical Kinetics and Equilibrium

Chemical 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 information

Ch 13 Chemical Kinetics. Modified by Dr. Cheng-Yu Lai

Ch 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 information

Lecture Presentation. Chapter 14. Chemical Kinetics. John D. Bookstaver St. Charles Community College Cottleville, MO Pearson Education, Inc.

Lecture 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 information

Chapter 12. Kinetics. Factors That Affect Reaction Rates. Factors That Affect Reaction Rates. Chemical. Kinetics

Chapter 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 information

Chemistry 1B, Fall 2016 Topic 23

Chemistry 1B, Fall 2016 Topic 23 Chemistry 1B Fall 016 [more] Chemical Kinetics 1 goals for topic 3 kinetics and mechanism of chemical reaction energy profile and reaction coordinate activation energy and temperature dependence of rate

More information

How 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 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 information

Chapter 12. Chemical Kinetics

Chapter 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 information

REACTION KINETICS. Catalysts substances that increase the rates of chemical reactions without being used up. e.g. enzymes.

REACTION KINETICS. Catalysts substances that increase the rates of chemical reactions without being used up. e.g. enzymes. REACTION KINETICS Study of reaction rates Why? Rates of chemical reactions are primarily controlled by 5 factors: the chemical nature of the reactants 2 the ability of the reactants to come in contact

More information

11/2/ and the not so familiar. Chemical kinetics is the study of how fast reactions take place.

11/2/ 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 information

Factors That Affect Rates. Factors That Affect Rates. Factors That Affect Rates. Factors That Affect Rates

Factors 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 information

Kinetics - Chapter 14. reactions are reactions that will happen - but we can t tell how fast. - the steps by which a reaction takes place.

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 information

Reaction Rates. Let's assume that this reaction does not occur instantaneously, and therefore, it takes some time

Reaction Rates. Let's assume that this reaction does not occur instantaneously, and therefore, it takes some time Chemical Kinetics Reaction Rates Up to this point in the course our concern with chemical equations has focused upon understanding, reactants, products, stoichiometry, and states. We have also looked at

More information

CHEMISTRY. Chapter 14 Chemical Kinetics

CHEMISTRY. 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 information

Take home Exam due Wednesday, Aug 26. In class Exam will be the that morning class multiple choice questions.

Take home Exam due Wednesday, Aug 26. In class Exam will be the that morning class multiple choice questions. Announcements Take home Exam due Wednesday, Aug 26. In class Exam will be the that morning class. 15-20 multiple choice questions. Updated projects Aug 28: answer what lab chemistry needs to get done to

More information

Chapter 14 Chemical Kinetics

Chapter 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 information

Chapter 14 Chemical Kinetics

Chapter 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 information

on-line kinetics 3!!! Chemistry 1B Fall 2013

on-line kinetics 3!!! Chemistry 1B Fall 2013 on-line kinetics 3!!! Chemistry 1B Fall 2013 1 on-line kinetics 3!!! Chemistry 1B Fall 2013 Mechanism of a chemical reaction Elementary reactions Activation energy and reaction coordinate diagram 2 Chemistry

More information

Chemical Kinetics. Rate = [B] t. Rate = [A] t. Chapter 12. Reaction Rates 01. Reaction Rates 02. Reaction Rates 03

Chemical 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 information

Chapter 13 Kinetics: Rates and Mechanisms of Chemical Reactions

Chapter 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 information

AP 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 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 information

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?

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? 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 information

Chemical 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 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 information

Chapter 11: CHEMICAL KINETICS

Chapter 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 information

14.1 Factors That Affect Reaction Rates

14.1 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 information

Chemistry 1B Fall 2016

Chemistry 1B Fall 2016 Chemistry 1B Fall 2016 Topic 23 [more] Chemical Kinetics 1 goals for topic 23 kinetics and mechanism of chemical reaction energy profile and reaction coordinate activation energy and temperature dependence

More information

Theoretical Models for Chemical Kinetics

Theoretical Models for Chemical Kinetics Theoretical Models for Chemical Kinetics Thus far we have calculated rate laws, rate constants, reaction orders, etc. based on observations of macroscopic properties, but what is happening at the molecular

More information

Lecture 22: The Arrhenius Equation and reaction mechanisms. As we wrap up kinetics we will:

Lecture 22: The Arrhenius Equation and reaction mechanisms. As we wrap up kinetics we will: As we wrap up kinetics we will: Lecture 22: The Arrhenius Equation and reaction mechanisms. Briefly summarize the differential and integrated rate law equations for 0, 1 and 2 order reaction Learn how

More information

Chemical. Chapter 14. Kinetics. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E.

Chemical. 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 information

Chemical Kinetics. Reaction Rate. Reaction Rate. Reaction Rate. Reaction Rate. Chemistry: The Molecular Science Moore, Stanitski and Jurs

Chemical Kinetics. Reaction Rate. Reaction Rate. Reaction Rate. Reaction Rate. Chemistry: The Molecular Science Moore, Stanitski and Jurs Chemical Kinetics Chemistry: The Molecular Science Moore, Stanitski and Jurs The study of speeds of reactions and the nanoscale pathways or rearrangements by which atoms and molecules are transformed to

More information

Chapter 14: Chemical Kinetics

Chapter 14: Chemical Kinetics C h e m i c a l K i n e t i c s P a g e 1 Chapter 14: Chemical Kinetics Homework: Read Chapter 14 Work out sample/practice exercises in the sections, Check for the MasteringChemistry.com assignment and

More information

Examples of fast and slow reactions

Examples 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 information

Outline: Kinetics. Reaction Rates. Rate Laws. Integrated Rate Laws. Half-life. Arrhenius Equation How rate constant changes with T.

Outline: 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 information

Chem 1B Objective 6: Describe reaction mechanisms and relate mechanism to rate law and reaction energy diagram.

Chem 1B Objective 6: Describe reaction mechanisms and relate mechanism to rate law and reaction energy diagram. Chem 1B Objective 6: Describe reaction mechanisms and relate mechanism to rate law and reaction energy diagram. Key Ideas: A reaction mechanism helps us understand how a reaction occurs. (E.g., drug companies

More information

Chapter 11 Rate of Reaction

Chapter 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 information

2013 W. H. Freeman and Company. 6 Enzymes

2013 W. H. Freeman and Company. 6 Enzymes 2013 W. H. Freeman and Company 6 Enzymes CHAPTER 6 Enzymes Key topics about enzyme function: Physiological significance of enzymes Origin of catalytic power of enzymes Chemical mechanisms of catalysis

More information

Reaction Rate. Rate = Conc. of A at t 2 -Conc. of A at t 1. t 2 -t 1. Rate = Δ[A] Δt

Reaction 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 information

Name AP CHEM / / Chapter 12 Outline Chemical Kinetics

Name 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 information

CHAPTER 13 (MOORE) CHEMICAL KINETICS: RATES AND MECHANISMS OF CHEMICAL REACTIONS

CHAPTER 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 information

Chapter 14 Chemical Kinetics

Chapter 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 information

How can we use the Arrhenius equation?

How can we use the Arrhenius equation? How can we use the Arrhenius equation? k = Ae Ea RT Lab H 3 CNC(g) H 3 CCN(g) 1. Experiment to determine rate law 2. Experiment to determine Ea Temperature (K) k (s -1 ) 1/T ln k 462.9 2.52E-05 0.00216-10.589

More information

Chapter 14. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten

Chapter 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 information

CHEMICAL KINETICS. (Part II)

CHEMICAL KINETICS. (Part II) Chapter 14 CHEMICAL KINETICS (Part II) Dr. Al Saadi 1 Reaction Mechanism Most reactions occur in a series of steps. The balancedequation equation gives information about the initial reactants and the final

More information

Chemical Kinetics Ch t ap 1 er

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 information

C H E M I C N E S C I

C 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 information

Shroud of Turin. Chemical Kinetics. Reaction Rates. Reaction Rates. Reaction Rates. Chemical Kinetics: The Rates of Chemical Reactions

Shroud of Turin. Chemical Kinetics. Reaction Rates. Reaction Rates. Reaction Rates. Chemical Kinetics: The Rates of Chemical Reactions Page III-12-1 / Chapter Twelve Lecture Notes Chemical Kinetics: The Rates of Chemical Reactions Chapter 12 Chemistry 222 Professor Michael Russell Shroud of Turin Shroud of Jesus?!? Fake or Real? Explored

More information

Chapter 12 - Chemical Kinetics

Chapter 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 information

Chapter 16. Rate Laws. The rate law describes the way in which reactant concentration affects reaction rate.

Chapter 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 information

Chemical Kinetics. What Influences Kinetics?

Chemical 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 information

Chemistry 1B, Fall 2012 Lecture 23

Chemistry 1B, Fall 2012 Lecture 23 Chemistry 1B Fall 01 [more] Chemical Kinetics 1 kinetics and mechanism of reaction NO (g) + CO(g) ô NO(g) + CO (g) at T< 500K if the reaction was a collision between a NO molecule and a CO molecule one

More information

11/9/2012 CHEMICAL REACTIONS. 1. Will the reaction occur? 2. How far will the reaction proceed? 3. How fast will the reaction occur?

11/9/2012 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 information

Chapter 13 Rates of Reactions

Chapter 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 information

Chemical Kinetics. Kinetics. Factors That Affect Reaction Rates. Factors That Affect Reaction Rates. Factors That Affect Reaction Rates

Chemical Kinetics. Kinetics. Factors That Affect Reaction Rates. Factors That Affect Reaction Rates. Factors That Affect Reaction Rates Kinetics hemical Kinetics In kinetics we study the rate at which a chemical process occurs. esides information about the speed at which reactions occur, kinetics also sheds light on the reaction mechanism

More information

SAMPLE 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 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 information

ALE 4. Effect of Temperature and Catalysts on the Rate of a Chemical Reaction

ALE 4. Effect of Temperature and Catalysts on the Rate of a Chemical Reaction Name Chem 163 Section: Team Number: ALE 4. Effect of Temperature and Catalysts on the Rate of a Chemical Reaction (Reference: 16.5 16.6 & 16.8 Silberberg 5 th edition) Why do reaction rates increase as

More information

Unit 12: Chemical Kinetics

Unit 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 information

Chem 112 PRACTICE EXAM 2 Adapted from Spring 2015 Kinetics, Thermo Part 1

Chem 112 PRACTICE EXAM 2 Adapted from Spring 2015 Kinetics, Thermo Part 1 Chem 112 PRACTICE EXAM 2 Adapted from Spring 2015 Kinetics, Thermo Part 1 1. When N 2 O 5 (g) decomposes as shown below at a fixed temperature, the rate of formation of NO 2 is 3.7 10 3 M/s. 2 N 2 O 5

More information

Chapter 30. Chemical Kinetics. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved.

Chapter 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 information

CHEM Dr. Babb s Sections Lecture Problem Sheets

CHEM Dr. Babb s Sections Lecture Problem Sheets CHEM 116 - Dr. Babb s Sections Lecture Problem Sheets Kinetics: Integrated Form of Rate Law 61. Give the integrated form of a zeroth order reaction. Define the half-life and find the halflife for a general

More information

Chemical 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 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 information

Chemistry 201: General Chemistry II - Lecture

Chemistry 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 information

Chemistry 1B, Fall 2016 Topic 23

Chemistry 1B, Fall 2016 Topic 23 Chemistry 1B, Fall 016 Topic 3 Chemistry 1B Fall 016 Topic 3 [more] Chemical Kinetics goals for topic 3 inetics and mechanism of chemical reaction energy profile and reaction coordinate activation energy

More information

CHEMISTRY - CLUTCH CH.13 - CHEMICAL KINETICS.

CHEMISTRY - 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 information

Chemical Kinetics. Topic 7

Chemical Kinetics. Topic 7 Chemical Kinetics Topic 7 Corrosion of Titanic wrec Casón shipwrec 2Fe(s) + 3/2O 2 (g) + H 2 O --> Fe 2 O 3.H 2 O(s) 2Na(s) + 2H 2 O --> 2NaOH(aq) + H 2 (g) Two examples of the time needed for a chemical

More information

Name: UNIT 5 KINETICS NOTES PACEKT #: KINETICS NOTES PART C

Name: UNIT 5 KINETICS NOTES PACEKT #: KINETICS NOTES PART C KINETICS NOTES PART C IV) Section 14.4 The Change of Concentration with Time A) Integrated Rate Law: shows how the concentration of the reactant(s) varies with time 1) [A]0 is the initial concentration

More information

Chemical Kinetics. What quantities do we study regarding chemical reactions? 15 Chemical Kinetics

Chemical Kinetics. What quantities do we study regarding chemical reactions? 15 Chemical Kinetics Chemical Kinetics Chemical kinetics: the study of reaction rate, a quantity conditions affecting it, the molecular events during a chemical reaction (mechanism), and presence of other components (catalysis).

More information

What is an enzyme? Lecture 12: Enzymes & Kinetics I Introduction to Enzymes and Kinetics. Margaret A. Daugherty Fall 2004 KEY FEATURES OF ENZYMES

What is an enzyme? Lecture 12: Enzymes & Kinetics I Introduction to Enzymes and Kinetics. Margaret A. Daugherty Fall 2004 KEY FEATURES OF ENZYMES Lecture 12: Enzymes & Kinetics I Introduction to Enzymes and Kinetics Margaret A. Daugherty Fall 2004 What is an enzyme? General Properties Mostly proteins, but some are actually RNAs Biological catalysts

More information

AP CHEMISTRY NOTES 7-1 KINETICS AND RATE LAW AN INTRODUCTION

AP 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 information

TOPIC 6: Chemical kinetics

TOPIC 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 information

14.4 Reaction Mechanism

14.4 Reaction Mechanism 14.4 Reaction Mechanism Steps of a Reaction Fred Omega Garces Chemistry 201 Miramar College 1 Reaction Mechanism The Ozone Layer Ozone is most important in the stratosphere, at this level in the atmosphere,

More information

Chemical kinetics and catalysis

Chemical kinetics and catalysis Chemical kinetics and catalysis Outline Classification of chemical reactions Definition of chemical kinetics Rate of chemical reaction The law of chemical raction rate Collision theory of reactions, transition

More information

CHAPTER 10 CHEMICAL KINETICS

CHAPTER 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 information