AP * Chemistry. Kinetics: Integrated Rate Law & Determining Ea. René McCormick

Size: px
Start display at page:

Download "AP * Chemistry. Kinetics: Integrated Rate Law & Determining Ea. René McCormick"

Transcription

1 AP * Chemistry Kinetics: Integrated Rate Law & Determining Ea René McCormick *AP is a registered trademark of the College Board, which was not involved in the production of, and does not endorse, this product by René McCormick. All rights reserved.

2

3 Kinetics These terms may be used in a question testing your understanding of KINETICS Rate; time; concentration; order; rate constant; mechanisms; rate determining step; intermediate; catalyst; halflife; instantaneous rate; relative rate; activation energy; integrated rate law; rate expression; rate law Key Formulas and Relationships Δ in some measurable quantity Rate = time and is measured in units of M time or M 1 time 1 Instantaneous rate: rate at an instant of time. Draw a line tangent to the curve of concentration vs. time and calculate the slope of the tangent line. Relative rate: Start with the balance equation, next make each coefficient in the balanced equation the denominator of a fraction and assign the numerator a value of 1. Now, all of the terms in the balanced chemical equation can be set relative to each other. Example: 2A + 3B C + 2D becomes 1 A+ 1 B C+ 1 D where it follows that ΔA 1 ΔB ΔC 1 ΔD rate = = =+ =+ 2 Δt 3 Δt Δt 2 Δt You ll only be asked to relate two terms to each other, not all of the terms that can be generated. Take caution to assign reactants a negative sign since they are disappearing and products a positive sign since they are appearing. Your clue as to when to use this is rate in terms of which is code for relative rates as well as statements such as: In experiment 2 or anything that asks about the rate of a different reactant or product than that listed in the table of concentration-rate data. Differential Rate Law (concentration vs. rate data): Rate = k [A] x [B] y and graphical methods are simplest. We linearize data to avoid calculus! Memorize the graphical pattern: Set up your axes so that time is always on the x-axis. Plot the concentration of the reactant on the y-axis of the first graph. Plot the natural log of the concentration (ln [A], NOT log[a]) on the y-axis of the second graph and the reciprocal of the concentration on the y-axis of the third graph. You are in search of linear data! Here comes the elegant part If you do the set of graphs in this order with the y-axes being concentration, natural log of concentration and reciprocal concentration, the alphabetical order of the y-axis variables leads to 0, 1, 2 orders respectively for that reactant. Zero order k = negative slope First order k = negative slope Second order k = the slope

4 You can now easily solve for either time or concentration once you know the order of the reactant. Just remember y = mx + b. Choose the set of variables that gave you the best straight line (r value closest to ±1) and insert them in place of x and y in the generalized equation for a straight line. A is reactant A and A o is the initial concentration of reactant A at time zero [the y-intercept]. y = mx + b zero order [A] = kt + [A o ] first order ln[a] = kt + ln [A o ] second order 1/[A] = kt + 1/[A o ] Also recognize that slope = k, since the rate constant is NEVER negative. If you are asked to write the rate order you determined from analyzing the graphs expression [or rate law] it is simply Rate = k[a] Also half-life plays a role in kinetics: t 1 = for first order reactions and all nuclear decay 2 k To calculate the activation energy we use the Arrhenius equation relates k and temperature: Ea 1 ln k = + ln A, so a graph of lnk vs. 1 R T T is linear and the E a = slope R( the energy R) Key Concepts Be able to explain with algebraic equations or words how an order is determined. It is important to state which concentration(s) is held constant and which concentration is varied as well the effect that has on the rate of the reaction if you choose not to justify with algebraic equations. Mechanisms must agree with the stoichiometry of the reaction and the summary rate law must agree up to and including the slow step; identify intermediates and catalysts and clearly state that the correct mechanism agrees with the experimentally determined rate law. Discuss number of effective collisions in relation to increasing or decreasing rates Arrhenius magnitude of k relates directly to the speed of the reaction; large = fast; small = slow E a also predicts speed but the relationship is an inverse one; high = slow rate; low = fast rate instantaneous rate = slope of the line tangent to the time point in question Connections to Other Chapters Stoichiometry -- using up one component of the system might indicate a limiting reactant in effect Electrochemistry -- if reaction is redox in nature you could be asked to bridge to this concept Potenial Pitfalls and Unit Warnings Units on k = always time -1 and one less M -1 than overall order. Ex: 2 nd order overall has a k with units of M -1 s -1 liter = = liter mol s = mol s M s

5 Figures or graphs you may need to interpret Change in [Conc] over time; notice stoich ratio in effect Instantaneous Rate Energy diagram; locate activation energy, overall energy, transition state, endo./exo, effect of adding a catalyst. Be able to evaluate energy quantities for BOTH the forward and reverse reactions. Zero Order First Order Second Order WHY increasing the temperature increases the rate of a reaction Arrhenius plot to determine activation energy E a = energy R slope Catalysts increase the rate of reaction by lowering the activation energy and providing an alternate mechanism

6 Kinetics Concept Map graph [A] vs. time graph ln[a] vs. time graph 1/[A] vs. time graph lnk vs. 1/[T] Page 9

7 2004 AP CHEMISTRY FREE-RESPONSE QUESTIONS 3. The first-order decomposition of a colored chemical species, X, into colorless products is monitored with a spectrophotometer by measuring changes in absorbance over time. Species X has a molar absorptivity constant of cm 1 M 1 and the path length of the cuvette containing the reaction mixture is 1.00 cm. The data from the experiment are given in the table below. [X] ( M ) Absorbance Time (min)? ? (a) Calculate the initial concentration of the colored species. (b) Calculate the rate constant for the first-order reaction using the values given for concentration and time. Include units with your answer. (c) Calculate the number of minutes it takes for the absorbance to drop from to (d) Calculate the half-life of the reaction. Include units with your answer. (e) Experiments were performed to determine the value of the rate constant for this reaction at various temperatures. Data from these experiments were used to produce the graph below, where T is temperature. This graph can be used to determine the activation energy, E a, of the reaction. (i) Label the vertical axis of the graph. (ii) Explain how to calculate the activation energy from this graph. STOP If you finish before time is called, you may check your work on this part only. Do not turn to the other part of the test until you are told to do so. Copyright 2004 by College Entrance Examination Board. All rights reserved. Visit apcentral.collegeboard.com (for AP professionals) and (for AP students and parents). Page 12

8 2005 AP CHEMISTRY FREE-RESPONSE QUESTIONS (Form B) X 2 Y + Z 3. The decomposition of gas X to produce gases Y and Z is represented by the equation above. In a certain experiment, the reaction took place in a 5.00 L flask at 428 K. Data from this experiment were used to produce the information in the table below, which is plotted in the graphs that follow. Time [X] [X] (minutes) (mol L 1 ln [X] ) (L mol 1 ) ,110 Copyright 2005 by College Entrance Examination Board. All rights reserved. Visit apcentral.collegeboard.com (for AP professionals) and (for AP students and parents). 8 GO ON TO THE NEXT PAGE. Page 13

9 2005 AP CHEMISTRY FREE-RESPONSE QUESTIONS (Form B) (a) How many moles of X were initially in the flask? (b) How many molecules of Y were produced in the first 20. minutes of the reaction? (c) What is the order of this reaction with respect to X? Justify your answer. (d) Write the rate law for this reaction. (e) Calculate the specific rate constant for this reaction. Specify units. (f) Calculate the concentration of X in the flask after a total of 150. minutes of reaction. STOP If you finish before time is called, you may check your work on this part only. Do not turn to the other part of the test until you are told to do so. Copyright 2005 by College Entrance Examination Board. All rights reserved. Visit apcentral.collegeboard.com (for AP professionals) and (for AP students and parents). 9 Page 14

AP* Kinetics Free Response Questions KEY page 1

AP* Kinetics Free Response Questions KEY page 1 AP* Kinetics Free Response Questions KEY page 1 Essay Questions 1983 a) three points Plot ln k or log k vs 1/T Eact = - R (slope) or - 2,303 R (slope) For partial credit, if the 2-point equation is given

More information

2005 AP CHEMISTRY FREE-RESPONSE QUESTIONS (Form B)

2005 AP CHEMISTRY FREE-RESPONSE QUESTIONS (Form B) 2005 AP CHEMISTRY FREE-RESPONSE QUESTIONS (Form B) 6. Consider two containers of volume 1.0 L at 298 K, as shown above. One container holds 0.10 mol N 2 (g) and the other holds 0.10 mol H 2 (g). The average

More information

AP CALCULUS AB 2006 SCORING GUIDELINES (Form B) Question 2. the

AP CALCULUS AB 2006 SCORING GUIDELINES (Form B) Question 2. the AP CALCULUS AB 2006 SCORING GUIDELINES (Form B) Question 2 Let f be the function defined for x 0 with f ( 0) = 5 and f, the ( x 4) 2 first derivative of f, given by f ( x) = e sin ( x ). The graph of y

More information

3: Chemical Kinetics Name: HW 6: Review for Unit Test KEY Class: Date: A Products

3: Chemical Kinetics Name: HW 6: Review for Unit Test KEY Class: Date: A Products 3: Chemical Kinetics Name: HW 6: Review for Unit Test KEY Class: Date: Page 1 of 9 AP Multiple Choice Review Questions 1 16 1. The reaction rate is defined as the change in concentration of a reactant

More information

NAME: Chapter 14Chemical Kinetics (Reaction Rate Law Concepts)

NAME: 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 information

2005 AP PHYSICS C: ELECTRICITY AND MAGNETISM FREE-RESPONSE QUESTIONS

2005 AP PHYSICS C: ELECTRICITY AND MAGNETISM FREE-RESPONSE QUESTIONS 2005 AP PHYSICS C: ELECTRICITY AND MAGNETISM In the circuit shown above, resistors 1 and 2 of resistance R 1 and R 2, respectively, and an inductor of inductance L are connected to a battery of emf e and

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

Calculations In Chemistry

Calculations In Chemistry Calculations In Chemistry Module 27 Kinetics: Rate Laws Module 27 Kinetics: Rate Laws...773 Lesson 27A: Kinetics Fundamentals...771 Lesson 27B: Rate Laws...778 Lesson 27C: Integrated Rate Law --Zero Order...787

More information

Kinetics CHAPTER IN THIS CHAPTER

Kinetics 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 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

Performance Task: Concentration vs. Time

Performance Task: Concentration vs. Time NAME DATE : Concentration vs. Time Goal of task Target concept: Understand reaction rates in both qualitative and quantitative terms For this task you will be evaluated on your ability to: Construct an

More information

AP* Electrochemistry Free Response Questions page 1

AP* Electrochemistry Free Response Questions page 1 Galvanic (Voltaic) Cells 1988 Average score = 5.02 a) two points Sn ---> Sn 2+ + 2e Ag + + e ---> Ag AP* Electrochemistry Free Response Questions page 1 b) two points 2 Ag + + Sn ---> 2 Ag + Sn 2+ E =

More information

Lecture 19: Introduction to Kinetics First a CH 302 Kinetics Study Guide (Memorize these first three pages, they are all the background you need)

Lecture 19: Introduction to Kinetics First a CH 302 Kinetics Study Guide (Memorize these first three pages, they are all the background you need) Lecture 19: Introduction to Kinetics First a CH 302 Kinetics Study Guide (Memorize these first three pages, they are all the background you need) Reaction Rate: The most important issue in kinetics is

More information

2005 AP CHEMISTRY FREE-RESPONSE QUESTIONS (Form B)

2005 AP CHEMISTRY FREE-RESPONSE QUESTIONS (Form B) 2005 AP CHEMISTRY FREE-RESPONSE QUESTIONS (Form B) Answer EITHER Question 2 below OR Question 3 printed on pages 8 and 9. Only one of these two questions will be graded. If you start both questions, be

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

Advanced Placement. Chemistry. Integrated Rates

Advanced Placement. Chemistry. Integrated Rates Advanced Placement Chemistry Integrated Rates 204 47.90 9.22 78.49 (26) 50.94 92.9 80.95 (262) 52.00 93.94 83.85 (263) 54.938 (98) 86.2 (262) 55.85 0. 90.2 (265) 58.93 02.9 92.2 (266) H Li Na K Rb Cs Fr

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

Chemical Reaction Rates II

Chemical Reaction Rates II 25 Solving Kinetics Problems Involving Integrated Rate Law Chemical kinetics is the study of the speed or rate of a chemical reaction under various conditions. Collisions must occur in order for chemical

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

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

AP* Physics B: Newton s Laws YOU MAY USE YOUR CALCULATOR

AP* Physics B: Newton s Laws YOU MAY USE YOUR CALCULATOR AP* Physics B: Newton s Laws Name: Period: YOU MAY USE YOUR CALCULATOR CLEARLY SHOW THE METHOD YOU USED AND STEPS INVOLVED IN ARRIVING AT YOUR ANSWERS. It is to your advantage to do this, because you may

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 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

2006 AP6 CALCULUS AB FREE-RESPONSE QUESTIONS

2006 AP6 CALCULUS AB FREE-RESPONSE QUESTIONS 2006 AP6 CALCULUS AB FREE-RESPONSE QUESTIONS dy 1+ y 5. Consider th e differential equation =, where x 0. dx x (a) On the axes provided, sketch a slope field for the given differential equation at the

More information

AP CALCULUS BC 2006 SCORING GUIDELINES (Form B) Question 2

AP CALCULUS BC 2006 SCORING GUIDELINES (Form B) Question 2 AP CALCULUS BC 2006 SCORING GUIDELINES (Form B) Question 2 An object moving along a curve in the xy-plane is at position ( x() t, y() t ) at time t, where dx t tan( e ) for t 0. At time t =, the object

More information

2/23/2018. Familiar Kinetics. ...and the not so familiar. Chemical kinetics is the study of how fast reactions take place.

2/23/2018. 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 information

Chemical Kinetics -- Chapter 14

Chemical 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 information

It must be determined from experimental data, which is presented in table form.

It 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 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

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 2011 SCORING GUIDELINES

AP CHEMISTRY 2011 SCORING GUIDELINES AP CHEMISTRY 2011 SCORING GUIDELINES Question 6 In an experiment, all the air in a rigid 2.0 L flask is pumped out. Then some liquid ethanol is injected into the sealed flask, which is held at 35 C. The

More information

Chapter 14: Chemical Kinetics

Chapter 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 information

Determination of the Rate of a Reaction, Its Order, and Its Activation Energy

Determination of the Rate of a Reaction, Its Order, and Its Activation Energy Determination of the Rate of a Reaction, Its Order, and Its Activation Energy Reaction kinetics is defined as the study of the rates of chemical reactions and their mechanisms. Reaction rate is simply

More information

AP CALCULUS AB 2004 SCORING GUIDELINES (Form B)

AP CALCULUS AB 2004 SCORING GUIDELINES (Form B) AP CALCULUS AB 004 SCORING GUIDELINES (Form B) Question 4 The figure above shows the graph of f, the derivative of the function f, on the closed interval 1 x 5. The graph of f has horizontal tangent lines

More information

AP CALCULUS BC 2015 SCORING GUIDELINES

AP CALCULUS BC 2015 SCORING GUIDELINES 05 SCORING GUIDELINES Question 5 Consider the function f =, where k is a nonzero constant. The derivative of f is given by k f = k ( k). (a) Let k =, so that f =. Write an equation for the line tangent

More information

Ch part 2.notebook. November 30, Ch 12 Kinetics Notes part 2

Ch 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 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

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

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

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

AP Questions: Kinetics

AP Questions: Kinetics AP Questions: Kinetics 1972 2 A + 2 B C + D The following data about the reaction above were obtained from three experiments: Rate of Formation of [A] [B] C (mole. liter -1 min -1 ) 1 0.60 0.15 6.3 10-3

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

Solutions - Practice Test - CHEM 112 Exam 1

Solutions - Practice Test - CHEM 112 Exam 1 Solutions - Practice Test - CHEM 112 Exam 1 1B. The rates of formation and decomposition are average rates that can be predicted by using the stoichiometry of the balanced equation to get: 1 D[ N 2O5 ]

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

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

Unit #10. Chemical Kinetics

Unit #10. Chemical Kinetics 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

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

U N I T T E S T P R A C T I C E

U N I T T E S T P R A C T I C E South Pasadena AP Chemistry Name 2 Chemical Kinetics Period Date U N I T T E S T P R A C T I C E Part 1 Multiple Choice You should allocate 30 minutes to finish this portion of the test. No calculator

More information

AP CALCULUS AB 2011 SCORING GUIDELINES (Form B)

AP CALCULUS AB 2011 SCORING GUIDELINES (Form B) 0 SCORING GUIDELINES (Form B) Consider a differentiable function f having domain all positive real numbers, and for which it is known that f = ( 4 x) x for x > 0. (a) Find the x-coordinate of the critical

More information

Chapter: Chemical Kinetics

Chapter: 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 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

EXPERIMENT 1 REACTION RATE, RATE LAW, AND ACTIVATION ENERGY THE IODINE CLOCK REACTION

EXPERIMENT 1 REACTION RATE, RATE LAW, AND ACTIVATION ENERGY THE IODINE CLOCK REACTION PURPOSE: To determine the Rate Law and the Activation Energy for a reaction from experimental data. PRINCIPLES: The Rate Law is a mathematical expression that predicts the rate of a reaction from the concentration

More 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 CALCULUS BC 2006 SCORING GUIDELINES (Form B) Question 6. n n n 3n

AP CALCULUS BC 2006 SCORING GUIDELINES (Form B) Question 6. n n n 3n AP CALCULUS BC 6 SCORING GUIDELINES (Form B) Question 6 The function f is defined by f ( ) =. The Maclaurin series for f is given by + 6 9 ( ) n n + + L+ + L, which converges to f ( ) for <

More information

concentrations (molarity) rate constant, (k), depends on size, speed, kind of molecule, temperature, etc.

concentrations (molarity) rate constant, (k), depends on size, speed, kind of molecule, temperature, etc. #73 Notes Unit 9: Kinetics and Equilibrium Ch. Kinetics and Equilibriums I. Reaction Rates NO 2(g) + CO (g) NO (g) + CO 2(g) Rate is defined in terms of the rate of disappearance of one of the reactants,

More information

Student Session Topic: Average and Instantaneous Rates of Change

Student Session Topic: Average and Instantaneous Rates of Change Student Session Topic: Average and Instantaneous Rates of Change The concepts of average rates of change and instantaneous rates of change are the building blocks of differential calculus. The AP exams

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

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

AP CALCULUS AB 2003 SCORING GUIDELINES

AP CALCULUS AB 2003 SCORING GUIDELINES CORING GUIDELINE Question Let R be the shaded region bounded by the graphs of y the vertical line =, as shown in the figure above. = and y = e and (b) Find the volume of the solid generated when R is revolved

More information

AP CALCULUS AB/CALCULUS BC 2017 SCORING GUIDELINES

AP CALCULUS AB/CALCULUS BC 2017 SCORING GUIDELINES AP CALCULUS AB/CALCULUS BC 07 SCORING GUIDELINES Question 4 H ( 0) = ( 9 7) = 6 4 H ( 0) = 9 An equation for the tangent line is y = 9 6 t. : slope : : tangent line : approimation The internal temperature

More information

AP CHEMISTRY 2008 SCORING GUIDELINES (Form B)

AP CHEMISTRY 2008 SCORING GUIDELINES (Form B) AP CHEMISTRY 2008 SCORING GUIDELINES (Form B) Question 2 A(g) + B(g) C(g) + D(g) For the gas-phase reaction represented above, the following experimental data were obtained. Experiment Initial [A] (mol

More information

AP CHEMISTRY 2009 SCORING GUIDELINES

AP CHEMISTRY 2009 SCORING GUIDELINES 2009 SCORING GUIDELINES Question 2 (10 points) A student was assigned the task of determining the molar mass of an unknown gas. The student measured the mass of a sealed 843 ml rigid flask that contained

More information

There is not enough activation energy for the reaction to occur. (Bonds are pretty stable already!)

There 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 information

Chemical Kinetics. System LENGTH: VOLUME MASS Temperature. 1 gal = 4 qt. 1 qt = in 3. 1 L = qt. 1 qt = L

Chemical Kinetics. System LENGTH: VOLUME MASS Temperature. 1 gal = 4 qt. 1 qt = in 3. 1 L = qt. 1 qt = L Chemical Kinetics Practice Exam Chemical Kinetics Name (last) (First) Read all questions before you start. Show all work and explain your answers to receive full credit. Report all numerical answers to

More information

AP* Bonding & Molecular Structure Free Response Questions page 1

AP* Bonding & Molecular Structure Free Response Questions page 1 AP* Bonding & Molecular Structure Free Response Questions page 1 Essay Questions 1991 a) two points ΔS will be negative. The system becomes more ordered as two gases orm a solid. b) two points ΔH must

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

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

Understanding Organic Reactions

Understanding Organic Reactions Understanding Organic Reactions Energy Diagrams For the general reaction: The energy diagram would be shown as: Understanding Organic Reactions Energy Diagrams Energy Diagrams Understanding Organic Reactions

More information

CHEMICAL KINETICS E + 2B 2C + D (1)

CHEMICAL KINETICS E + 2B 2C + D (1) CHEMICAL KINETICS Chemical kinetics is the branch of chemistry that is concerned with the study of the rates and mechanisms of chemical reactions. The rate of a reaction is a measure of its speed. Consider

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

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

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

Chapter 13 - Chemical Kinetics II. Integrated Rate Laws Reaction Rates and Temperature

Chapter 13 - Chemical Kinetics II. Integrated Rate Laws Reaction Rates and Temperature Chapter 13 - Chemical Kinetics II Integrated Rate Laws Reaction Rates and Temperature Reaction Order - Graphical Picture A ->Products Integrated Rate Laws Zero Order Reactions Rate = k[a] 0 = k (constant

More information

AP * Calculus Review. Limits, Continuity, and the Definition of the Derivative

AP * Calculus Review. Limits, Continuity, and the Definition of the Derivative AP * Calculus Review Limits, Continuity, and the Definition of the Derivative Teacher Packet Advanced Placement and AP are registered trademark of the College Entrance Examination Board. The College Board

More information

Reading, etc. Introduction to Chemical Kinetics. Energy profile for a reaction. The reverse direction... Reaction Rates.

Reading, etc. Introduction to Chemical Kinetics. Energy profile for a reaction. The reverse direction... Reaction Rates. Reading, etc. Introduction to Chemical Kinetics CHEM 7 T. Hughbanks Kinetics, Chapter Read and understand section., but the material is mainly for your edification. Read.2 -.6. Sections.7.8 are descriptive,

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

X + Ω --> Φ (1) 5X + 3Ω --> 2Φ (3) d[φ]/dt = -d(2/5)[x]/dt = -d(2/3)[ω]/dt (4)

X + Ω --> Φ (1) 5X + 3Ω --> 2Φ (3) d[φ]/dt = -d(2/5)[x]/dt = -d(2/3)[ω]/dt (4) CHEMICAL KINETICS OVERVIEW Reaction rates are seldom related to thermodynamic functions of state of reactants and products. What determines the rate are the properties of the reactants and the intermediate

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

Chapter 15: Phenomena

Chapter 15: Phenomena Chapter 5: Phenomena Phenomena: The reaction A(aq) + B(aq) C(aq) was studied at two different temperatures (298 K and 350 K). For each temperature the reaction was started by putting different concentrations

More information

Chem 401 Unit 1 (Kinetics & Thermo) Review

Chem 401 Unit 1 (Kinetics & Thermo) Review KINETICS 1. For the equation 2 H 2(g) + O 2(g) 2 H 2 O (g) How is the rate of formation of H 2 O mathematically related to the rate of disappearance of O 2? 1 Δ [H2O] Δ[O 2] = 2 Δt Δt 2. Determine the

More information

AP CALCULUS BC 2002 SCORING GUIDELINES (Form B)

AP CALCULUS BC 2002 SCORING GUIDELINES (Form B) SCORING GUIDELINES (Form B) Question )F=HJE?ALAIEJDANOF=AIJD=JEJIFIEJE=J=OJEAJBHГ > J > EICELA>O NJ IE! J=@OJ J = 5AJ?DJDAF=JDBJDAF=HJE?AEJDANOF=AFHLE@A@@E?=JAJDA@EHA?JEBJE =CJDAF=JD >.E@JDAH=CABNJ =@JDAH=CABOJ?.E@JDAI=AIJFIEJELAL=KABJBHMDE?DJDAN?H@E=JABJDAF=HJE?AEI=?=

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

Rate of Reaction. Introduction

Rate of Reaction. Introduction 5 Rate of Reaction Introduction This experiment will allow you to study the effects of concentration, temperature, and catalysts on a reaction rate. The reaction whose rate you will study is the oxidation

More information

Lab Report Rate of Chemical Reaction: The Iodination of Acetone

Lab Report Rate of Chemical Reaction: The Iodination of Acetone Abstract Lab Report Rate of Chemical Reaction: The Iodination of Acetone Members (Section 2): Nattanit Trakullapphan Thaksaporn Sirichanyaphong Narissara Pracharktam The only way to determine the rate

More information

Kinetics Practice Test 2017 Name: date: 1. Use the data provided the answer the question.

Kinetics Practice Test 2017 Name: date: 1. Use the data provided the answer the question. Kinetics Practice Test 2017 Name: date: 1. Use the data provided the answer the question. The data above was obtained for a reaction in which X + Y Z. Which of the following is the rate law for the reaction?

More 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

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 14 Homework Answers

Chapter 14 Homework Answers Chapter 14 Homework Answers 14.47 The slope of the tangent to the curve at each time is the negative of the rate at each time: Rate 60 = 8.5 10 4 mol L 1 s 1 Rate 120 = 4.0 10 4 mol L 1 s 1 14.49 From

More information

, but bursts into flames in pure oxygen.

, 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 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

AP CALCULUS BC 2008 SCORING GUIDELINES

AP CALCULUS BC 2008 SCORING GUIDELINES AP CALCULUS BC 2008 SCORING GUIDELINES Question 4 A particle moves along the x-axis so that its velocity at time t, for 0 t 6, is given by a differentiable function v whose graph is shown above. The velocity

More information

v AB + C à AC + B Ø Bonds breaking

v AB + C à AC + B Ø Bonds breaking Chemistry Study Guide 3 v Kinetics reaction rates Ø Catalyst Ø Temperature Ø Concentration Ø Bonds Ø Surface area v Kinetics Ø Kinetic energy is directly proportional to the temperature Ø Gasses will react

More information

Page 1. (b) A system at equilibrium will shift from its equilibrium position if:

Page 1. (b) A system at equilibrium will shift from its equilibrium position if: Page 1 1. Circle the correct answer (1 8 pts total) ( points each) (a) The rate constant for a reaction will change if: i) a catalyst is added ii) the concentration of reactants is increased iii) T is

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

Dr. Zellmer Chemistry 1220 Monday Time: 18 mins Spring Semester 2019 February 4, 2019 Quiz III. Name KEY Rec. TA/time

Dr. Zellmer Chemistry 1220 Monday Time: 18 mins Spring Semester 2019 February 4, 2019 Quiz III. Name KEY Rec. TA/time Dr. Zellmer Chemistry 1220 Monday Time: 18 mins Spring Semester 2019 February 4, 2019 Quiz III Name KEY Rec. TA/time 1. (8 pts) For the following reaction K P = 0.0752 at 480.0 EC. 2 Cl 2 (g) + 2 H 2 O

More information

AP Chemistry: General & Solubility Equilibrium

AP Chemistry: General & Solubility Equilibrium AP Chemistry: General & Solubility Equilibrium AgCl Ag Cl = 1.8 10 = [ x][ x] = x sp 10 2 x = [Ag ] = [Cl ] = molar solubility of AgCl = 1.3 10 5 René McCormick AP IS A REGISTERED TRADEMAR OF THE COLLEGE

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

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

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

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