Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemical Kinetics The area of chemistry that concerns reaction rates.

Slides:



Advertisements
Similar presentations
Chemical Kinetics Reaction rate - the change in concentration of reactant or product per unit time.
Advertisements

Chapter 12 Chemical Kinetics
Chapter 14 Chemical Kinetics In kinetics we study the rate at which a chemical process occurs. Lecture Presentation © 2012 Pearson Education, Inc.
CHAPTER 12: KINETICS Dr. Aimée Tomlinson Chem 1212.
Chapter 14 Chemical Kinetics *concerned with speed or rates of chemical reactions reaction rate- the speed at which a chemical reaction occurs reaction.
Overview of Ch Properties of Solutions Chapter 11.
Chemical Kinetics. CA Standards Collision Model Collisions must have enough energy to produce the reaction (must equal or exceed the activation energy).Collisions.
Reaction Rates And Chemical equilibrium. Chemical Kinetics The area of chemistry that concerns reaction rates. However, only a small fraction of collisions.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemical Kinetics The area of chemistry that concerns reaction rates.
Prentice Hall © 2003Chapter 14 Chapter 14 Chemical Kinetics CHEMISTRY The Central Science 9th Edition David P. White.
Reaction Rate Change in concentration of a reactant or product per unit time. [A] means concentration of A in mol/L; A is the reactant or product being.
Chapter 14 Chemical Kinetics
Chapter 12 Chemical Kinetics. Chapter 12 Table of Contents Copyright © Cengage Learning. All rights reserved Reaction Rates 12.2 Rate Laws: An.
Chapter 15 Kinetics. Kinetics Deals with the rate of chemical reactions Deals with the rate of chemical reactions Reaction mechanism – steps that a reaction.
Chemical Kinetics Unit 11.
Reaction Mechanism The reaction mechanism is the series of elementary steps by which a chemical reaction occurs.  The sum of the elementary steps must.
8–1 John A. Schreifels Chemistry 212 Chapter 14-1 Chapter 14 Rates of Reaction.
Chemical Kinetics Chapter 16. Chemical Kinetics Thermodynamics – does a reaction take place? Kinetics – how fast does a reaction proceed? Reaction rate.
Chemical Kinetics: Rates and Mechanisms of Chemical Reactions General Chemistry: An Integrated Approach Hill, Petrucci, 4 th Edition Mark P. Heitz State.
Ch 15 Rates of Chemical Reactions Chemical Kinetics is a study of the rates of chemical reactions. Part 1 macroscopic level what does reaction rate mean?
Chemical Kinetics Chapter 16. Kinetics Reaction Rates Factors affecting rate Quantitative rate expressions DeterminationFactors Models for Rates Reaction.
Chapter 15 Rates of Reaction.
Chemical Kinetics The area of chemistry that concerns reaction rates and reaction mechanisms.
Chapter 12 Chemical Kinetics. Chapter 12 Table of Contents Copyright © Cengage Learning. All rights reserved Reaction Rates 12.2 Rate Laws: An.
Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chemical Kinetics Chapter 13.
Chapter 12 Chemical Kinetics.
Chapter 12 Chemical Kinetics. Chapter 12 Table of Contents Copyright © Cengage Learning. All rights reserved Reaction Rates 12.2 Rate Laws: An.
Chemical Kinetics Chapter 12. Chemical Kinetics The area of chemistry that concerns reaction rates.
1 Chemical Kinetics The area of chemistry that concerns reaction rates. The area of chemistry that concerns reaction rates.
Reaction Rate Change in concentration of a reactant or product per unit time. [A] means concentration of A in mol/L; A is the reactant or product being.
Chapter 14 Chemical Kinetics. Review Section of Chapter 14 Test Net Ionic Equations.
Chemical Kinetics The area of chemistry that concerns reaction rates and reaction mechanisms.
Chapter 14 Chemical Kinetics. Review Section of Chapter 14 Test Net Ionic Equations.
Chemical Kinetics Kinetics – how fast does a reaction proceed?
Chemical Kinetics Chapter 13 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
1 Reaction Mechanism The series of steps by which a chemical reaction occurs. A chemical equation does not tell us how reactants become products - it is.
1 Chapter 12 – Chemical Kinetics 1.Second order Rate Law 2.Zero Order Rate Law 3.Reaction Mechanism 4.Model for Chemical Kinetics 5.Collision 6.Catalysis.
1 Chemical Kinetics Chapter 14 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
AP CHEMISTRY CHAPTER 12 KINETICS. 2 Chemical Kinetics Thermodynamics tells us if a reaction can occur Kinetics tells us how quickly the reaction occurs.
Chapter 14 – Chemical Kinetics The rate of a chemical reaction is the speed at which products or formed and reactants broken down. There factors that affect.
Chemical Kinetics Rates of Reactions ©2011 University of Illinois Board of Trustees
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry FIFTH EDITION by Steven S. Zumdahl University of Illinois.
Chemical Kinetics Chapter 13. Chemical Kinetics Thermodynamics – does a reaction take place? Kinetics – how fast does a reaction proceed? Reaction rate.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemical Kinetics The area of chemistry that concerns reaction rates.
Chemical Kinetics By: Ms. Buroker. Chemical Kinetics Spontaneity is important in determining if a reaction occurs- but it doesn’t tell us much about the.
Chemical Kinetics Chung (Peter) Chieh Professor of chemistry University of Waterloo Waterloo, Ontario, Canada Chung (Peter) Chieh University of Waterloo.
Chemical Kinetics. Collision Theory of Reactions Collision theory is simple - for a reaction to occur, particles must collide successfully! A successful.
Chpt 12 - Chemical Kinetics Reaction Rates Rate Laws Reaction Mechanisms Collision Theory Catalysis HW set1: Chpt 12 - pg , # 22, 23, 28 Due Jan.
CHEMICAL KINETICS Chapter 12.
How fast chemical reactions proceed How chemical reactions occur.
Kinetics Cartoon courtesy of NearingZero.net ©2011 University of Illinois Board of Trustees
Chemical Kinetics The speed with which chemical reactions occur depends on external conditions The area of chemistry concerned with the speed at which.
Chemical Kinetics Chapter 13 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Kinetics Big Idea 4: Rates of chemical reactions are determined by details of the molecular collisions.
Chemical Kinetics The area of chemistry that concerns reaction rates and reaction mechanisms.
Kinetics. Reaction Rate  Reaction rate is the rate at which reactants disappear and products appear in a chemical reaction.  This can be expressed as.
Chemical Kinetics. Kinetics The study of reaction rates. Spontaneous reactions are reactions that will happen - but we can’t tell how fast. (Spontaneity.
16-1 KINETICS: RATES AND MECHANISMS OF CHEMICAL REACTIONS.
slideshttp:\\academicstaff.kmu.ac.ir\aliasadipour1.
AP CHEMISTRY Chapter 14 Chemical Kinetics Chemical Kinetics Study of how rapidly a reaction will occur. In addition to speed of reaction, kinetics.
CHAPTER 14: KINETICS Dr. Aimée Tomlinson Chem 1212.
Chemical Kinetics Unit 10 – Chapter 12.
Rates of Reactions Chapter 6
Reaction Mechanism The reaction mechanism is the series of elementary steps by which a chemical reaction occurs. The sum of the elementary steps must give.
Chemical Kinetics The area of chemistry that concerns reaction rates and reaction mechanisms.
Reaction Mechanism Most chemical reactions occur by a series of elementary steps. An intermediate is formed in one step and used up in a subsequent step.
Chapter 14 Chemical Kinetics
Chemical Kinetics Lesson 2
Presentation transcript:

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemical Kinetics The area of chemistry that concerns reaction rates.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 2 Factors affecting reactions The commercial use of a chemical reaction requires knowledge of three factors: Stoichiometry Thermodynamics Kinetics

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 3 Kinetics Kinetics describes how fast reactants are used up and products are formed. Some reactions occur very fast (combustion) while others proceed very slowly (rusting). To be useful, reactions musty occur at a reasonable rate.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 4 Reaction Rate Change in concentration (conc) of a reactant or product per unit time.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 5 Example 1 Consider the following reaction: CO + NO 2 → CO 2 + NO At t 1 (0 seconds) [CO] = mol/L At t 2 (12.5 seconds) [CO] = mol/L (the brackets [ ] indicate concentration) Average rate = -∆[CO] = - [CO] 2 – [CO] 1 ∆t t 2 – t 1

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 6 Example 1 = mol/L – mol/L 12.5 s = mol/L∙s

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 7 General form For A + B → C + D Average reaction rate = - ∆[A] = - ∆[B] = ∆[C] = ∆[D] ∆t ∆t ∆t ∆t Expressed in terms of each reactant.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 8 Collision theory Particles must collide Particles must collide with the correct orientation. Particles must collide with sufficient energy.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 9 Factors affecting reaction rates Surface area Concentration Temperature Presence of a catalyst

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 10 Rate laws Must always be obeyed or you will be arrested by the kinetics police A mathematical expression that relates reaction rates to the concentration of reactants. The reaction order mathematically defines the extent to which the reaction rate depends on the concentrations of the reactants.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 11 Rate Laws Rate = k[NO 2 ] n k = rate constant n = rate order

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 12 Rate law expression For aA + bB → cC + dD Rate = k[A] m [B] n m ≠ a and n ≠ b The rate constant k must be determined experimentally. As the concentration of reactants change, the rate also changes.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 13 Rate law expressions The rate constant = k [A] = concentration of A [B] = concentration of B m = order of the reaction with respect to A n = order of the reaction with respect to B m + n = overall order of the reaction

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 14 Rate constant k Its value is for a specific reaction Its units depend on the overall order of the reaction Its value does not change with concentration Its value does not change over time Changes with temperature. Must be experimentally determined Depends upon the presence of a catalyst

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 15 Order of reaction For A + B → C + D Rate = k[A] m [B] n If the rate of the reaction is directly proportional to a change in [A] then the reaction is 1 st order (with respect to A) and m = 1 If the rate of the reaction does not change with [A], then the reaction is 0 order with respect to A. m = 0 The overall rate of the reaction is m + n

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 16 example 2NO + O 2 → 2NO 2 Rate = k[NO] 2 [O 2 ] This reaction is 2 nd order with respect to [NO] and 1 st order with respect to [O 2 ] The overall order of the reaction is 3 If you double the concentration of NO, the rate will quadruple (2 2 = 4) If you double the concentration of O 2 the rate of the reaction also doubles.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 17 Determining rate laws 2NO + H 2 → N 2 + 2H 2 O Trial #Initial [NO] Mol/L Initial [H 2 ] Mol/L Rate mol/L∙S 14.0 × × × × × × × × 10 -5

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 18 Determining rate laws Rate = k[NO] m [H 2 ] n We want to determine m and n m = 2 n = 1 The overall order of the reaction is 3 The rate law expression is k[NO] 2 [H 2 ]

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 19 Types of Rate Laws Differential Rate Law: expresses how rate depends on concentration. Integrated Rate Law: expresses how concentration depends on time.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 20 Example CH 3 CHO → CH 4 + CO trial[CH 3 CHO]Rate Mol/L∙S

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 21 Example A + 2B → AB 2 trial[A][B]Rate mol/L∙S 10.01M 1.5 × M0.02M1.5 × M0.03M6.0 × 10 -4

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 22 Example 2A + B 2 +C → D Trial #[A][B 2 ][C]Rate mol/L∙s × × × ×10 4

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 23 Example (cont.) Rate = k[A] x [B 2 ] y [C] z By inspection x = 2 Solve for y Use trial 1 and 4 since [C] does not change Rate 4 = k[A] 2 4 [B 2 ] y 4 [C] z 4 Rate 1 k[A] 2 1 [B 2 ] y 1 [C] z 1

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 24 Example (continued) 8.00 ×10 4 = (.04/.01) 2 × (.02/.01) y 1.25× = 16 × 2 y 2 y = 64/16 = 4 y = 2 Now solve for z

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 25 Example (continued) Use trial 1 and 3 because [B] does not change Rate 3 = k[A] 2 3 [C] z 3 Rate 1 k[A] 2 1 [C] z ×10 4 = (.03/.01) 2 × (.05/.01) z 1.250× = 9(5) z 5 z = 1 Z = 0

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 26 Example continued Rate = k[A] 2 [B 2 ] 2 k = rate/[A] 2 [B 2 ] 2 k = 1.25×10 3 / (.01) 2 (.01) 2 k = 1.25×10 11 L 3 /mol 3 ∙s Rate = 1.25×10 11 [A] 2 [B 2 ] 2

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 27 Method of Initial Rates Initial Rate: the “instantaneous rate” just after the reaction begins. The initial rate is determined in several experiments using different initial concentrations.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 28 Overall Reaction Order Sum of the order of each component in the rate law. rate = k[H 2 SeO 3 ][H + ] 2 [I  ] 3 The overall reaction order is = 6.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 29 First-Order Rate Law Integrated first-order rate law is ln[A] =  kt + ln[A] o For aA  Products in a 1st-order reaction,

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 30 Half-Life of a First-Order Reaction t 1/2 = half-life of the reaction k = rate constant For a first-order reaction, the half-life does not depend on concentration.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 31 Second-Order Rate Law For aA  products in a second-order reaction, Integrated rate law is

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 32 Half-Life of a Second-Order Reaction t 1/2 = half-life of the reaction k = rate constant A o = initial concentration of A The half-life is dependent upon the initial concentration.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 33 A Summary 1.Simplification: Conditions are set such that only forward reaction is important. 2.Two types: differential rate law integrated rate law 3.Which type? Depends on the type of data collected - differential and integrated forms can be interconverted.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 34 A Summary (continued) 4.Most common: method of initial rates. 5.Concentration v. time: used to determine integrated rate law, often graphically. 6.For several reactants: choose conditions under which only one reactant varies significantly (pseudo first-order conditions).

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 35 Reaction Mechanism 4 The series of steps by which a chemical reaction occurs. 4 A chemical equation does not tell us how reactants become products - it is a summary of the overall process.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 36 Reaction Mechanism (continued) 4 The reaction has many steps in the reaction mechanism.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 37 Often Used Terms Intermediate: formed in one step and used up in a subsequent step and so is never seen as a product. Molecularity: the number of species that must collide to produce the reaction indicated by that step. Elementary Step: A reaction whose rate law can be written from its molecularity. uni, bi and termolecular

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 38 Rate-Determining Step In a multistep reaction, it is the slowest step. It therefore determines the rate of reaction.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 39 Collision Model Key Idea: Molecules must collide to react. However, only a small fraction of collisions produces a reaction. Why? Arrhenius: An activation energy must be overcome.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 40 Transition state theory In a chemical reaction, the reactants must pass through a short-lived, high energy intermediate state called a transition state, before any products are formed. Activation energy is energy which must be absorbed by the reactants in the ground state to allow them to reach the transition state.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 41 Transition state theory continued If the energy of the products (E p ) is greater than the energy of the reactants (E r ), then the process is endothermic. If E p < E r then the reaction is exothermic.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 42 Arrhenius Equation 4 Collisions must have enough energy to produce the reaction (must equal or exceed the activation energy). 4 Orientation of reactants must allow formation of new bonds.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 43 Arrhenius Equation (continued) k = rate constant A = frequency factor E a = activation energy T = temperature R = gas constant

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 44 Catalysis Catalyst: A substance that speeds up a reaction without being consumed Enzyme: A large molecule (usually a protein) that catalyzes biological reactions. Homogeneous catalyst: Present in the same phase as the reacting molecules. Heterogeneous catalyst: Present in a different phase than the reacting molecules.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 45 Heterogeneous Catalysis 1. Adsorption and activation of the reactants. 2. Migration of the adsorbed reactants on the surface. 3. Reaction of the adsorbed substances. 4. Escape, or desorption, of the products. Steps: