THE COLLISION THEORY OF REACTION RATES
|
|
- Harold Wilkins
- 5 years ago
- Views:
Transcription
1 THE COLLISION THEORY OF REACTION RATES This page describes the collision theory of reaction rates. It concentrates on the key things which decide whether a particular collision will result in a reaction - in particular, the energy of the collision, and whether or not the molecules hit each other the right way around (the orientation of the collision). The individual factors which affect the rate of a reaction (temperature, concentration, and so on) are discussed on separate pages. You can get at these via the rates of reaction menu - there is a link at the bottom of the page. We are going to look in detail at reactions which involve a collision between two species. Species: This is a useful term which covers any sort of particle you like - molecule, ion, or free radical Reactions where a single species falls apart in some way are slightly simpler because you won't be involved in worrying about the orientation of collisions. Reactions involving collisions between more than two species are going to be extremely uncommon (see below). Reactions involving collisions between two species It is pretty obvious that if you have a situation involving two species they can only react together if they come into contact with each other. They first have to collide, and then they may react. Why "may react"? It isn't enough for the two species to collide - they have to collide the right way around, and they have to collide with enough energy for bonds to break. (The chances of all this happening if your reaction needed a collision involving more than 2 particles are remote. All three (or more) particles would have to arrive at exactly the same point in space at the same time, with everything lined up exactly right, and having enough energy to react. That's not likely to happen very often!) The orientation of collision Consider a simple reaction involving a collision between two molecules - ethene, CH 2 =CH 2, and hydrogen chloride, HCl, for example. These react to give chloroethane. As a result of the collision between the two molecules, the double bond between the two carbons is converted into a single bond. A hydrogen atom gets attached to one of the carbons and a chlorine atom to the other. Diagram 1 The reaction can only happen if the hydrogen end of the H-Cl bond approaches the carbon-carbon double bond. Any other collision between the two molecules doesn't work. The two simply bounce
2 off each other. Of the collisions shown in the diagram, only collision 1 may possibly lead on to a reaction. If you haven't read the page about the mechanism of the reaction, you may wonder why collision 2 won't work as well. The double bond has a high concentration of negative charge around it due to the electrons in the bonds. The approaching chlorine atom is also slightly negative because it is more electronegative than hydrogen. The repulsion simply causes the molecules to bounce off each other. In any collision involving unsymmetrical species, you would expect that the way they hit each other will be important in deciding whether or not a reaction happens. Diagram 2 The energy of the collision Activation Energy Even if the species are orientated properly, you still won't get a reaction unless the particles collide with a certain minimum energy called the activation energy of the reaction. Activation energy is the minimum energy required before a reaction can occur. You can show this on an energy profile for the reaction. For a simple over-all exothermic reaction, the energy profile looks like this: If the particles collide with less energy than the activation energy, nothing important happens. They bounce apart. You can think of the activation energy as a barrier to the reaction. Only those collisions which have energies equal to or greater than the activation energy result in a reaction. Any chemical reaction results in the breaking of some bonds (needing energy) and the making of new ones (releasing energy). Obviously some bonds have to be broken before new ones can be made. Activation energy is involved in breaking some of the original bonds. Where collisions are relatively gentle, there isn't enough energy available to start the bond-breaking process, and so the particles don't react. The Maxwell-Boltzmann Distribution Diagram 3 Because of the key role of activation energy in deciding whether a collision will result in a reaction, it would obviously be useful to know what sort of proportion of the particles present have high enough energies to react when they collide. In any system, the particles present will have a very wide range of energies. For gases, this can be shown on a graph called the Maxwell-Boltzmann Distribution which is a plot of the number of particles having each particular energy.
3 The area under the curve is a measure of the total number of particles present. The Maxwell-Boltzmann Distribution and activation energy Diagram 4 Remember that for a reaction to happen, particles must collide with energies equal to or greater than the activation energy for the reaction. We can mark the activation energy on the Maxwell-Boltzmann distribution: Notice that the large majority of the particles don't have enough energy to react when they collide. To enable them to react we either have to change the shape of the curve, or move the activation energy further to the left. This is described on other pages. THE EFFECT OF CATALYSTS ON REACTION RATES This page describes and explains the way that adding a catalyst affects the rate of a reaction. It assumes that you are already familiar with basic ideas about the collision theory of reaction rates, and with the Maxwell-Boltzmann distribution of molecular energies in a gas. Note that this is only a preliminary look at catalysis as far as it affects rates of reaction. If you are looking for more detail, there is a separate section dealing with catalysts which you can access via a links at the bottom of the page. The facts What are catalysts? A catalyst is a substance which speeds up a reaction, but is chemically unchanged at the end of the reaction. When the reaction has finished, you would have exactly the same mass of catalyst as you had at the beginning. Some examples Some common examples which you may need for other parts of your syllabus include: reaction Decomposition of hydrogen peroxide catalyst manganese(iv) oxide, MnO 2
4 Nitration of benzene Manufacture of ammonia by the Haber Process Conversion of SO 2 into SO 3 during the Contact Process to make sulphuric acid Hydrogenation of a C=C double bond concentrated sulphuric acid iron vanadium(v) oxide, V 2 O 5 nickel The explanation The key importance of activation energy Collisions only result in a reaction if the particles collide with enough energy to get the reaction started. This minimum energy required is called the activation energy for the reaction. Diagram 5 You can mark the position of activation energy on a Maxwell-Boltzmann distribution to get a diagram like this: Only those particles represented by the area to the right of the activation energy will react when they collide. The great majority don't have enough energy, and will simply bounce Diagram 6 apart. Catalysts and activation energy To increase the rate of a reaction you need to increase the number of successful collisions. One possible way of doing this is to provide an alternative way for the reaction to happen which has a lower activation energy. In other words, to move the activation energy on the graph like this: Adding a catalyst has exactly this effect on activation energy. A catalyst provides an alternative route for the reaction. That
5 alternative route has a lower activation energy. Showing this on an energy profile: A word of caution! Be very careful if you are asked about this in an exam. The correct form of words is "A catalyst provides an alternative route for the reaction with a lower activation energy." It does not "lower the activation energy of the reaction". There is a subtle difference between the two statements that is easily illustrated with a simple analogy. Suppose you have a mountain between two valleys so that the only way for people to get from one valley to the other is over the mountain. Only the most active people will manage to get from one valley to the other. Now suppose a tunnel is cut through the mountain. Many more people will now manage to get from one valley to the other by this easier route. You could say that the tunnel route has a lower activation energy than going over the mountain. But you haven't lowered the mountain! The tunnel has provided an alternative route but hasn't lowered the original one. The original mountain is still there, and some people will still choose to climb it. In the chemistry case, if particles collide with enough energy they can still react in exactly the same way as if the catalyst wasn't there. It is simply that the majority of particles will react via the easier catalysed route. Articles from accessed on 2/23/09
6 AP Chemistry Chemical Kinetics Introduction Name Questions about The Collision Theory of Reaction Rates 1. First a bit of review. What are the four factors that can affect the rate of a chemical reaction? 2. In the middle of the first page, the statement is made that molecules first have to collide, and then they may react. What two things must be true about that collision in order for the molecules to react? 3. Reactions involving two molecules colliding in order to react are said to be bimolecular. Reactions involving three molecules colliding in order to react are called termolecular and are exceptionally rare. Why? 4. Sketch and label diagram 2. It s kind of an important diagram, so it s worth knowing it well. 5. Define the term activation energy. 6. What happens if particles collide without sufficient activation energy? 7. Which types of reactions require activation energy to proceed? 8. If we could calculate the average energy of a molecule in diagram 3, what would that value be called?
7 A Very Few Questions about The Effect of Catalysts on Reaction Rates 9. Copy and label diagram Adjust your just-drawn diagram to show what happens when a catalyst is added to a reaction. 11. The statement that a catalyst lowers the activation energy of a reaction is incorrect. What is the more correct but related statement about what a catalyst does? 12. Explain in your own words, of course the mountain/tunnel analogy used on the last page of the article and how it relates to catalysis. From neither article 13. Most reactions do not happen in one step. Instead, they happen in multiple steps. For example in the upper atmosphere, ozone is destroyed in this process. step 1 Cl + O 3 à ClO + O 2 step 2 ClO + O à Cl + O 2 What is the overall reaction taking place? 14. In the reaction from #13, what substance is the catalyst - the thing that is consumed then remade at the end? 15. What substance is an intermediate being made in one step then consumed in a later step?
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 informationCollision Theory of Reaction Rates
Collision Theory of Reaction Rates If you have two reactants, they can only react if they come into contact with each other i.e. if they collide Then, they MAY react Why May? Collision alone is not enough
More informationTYPES OF CATALYSIS Reading Supplement
TYPES OF CATALYSIS Reading Supplement This page looks at the the different types of catalyst (heterogeneous and homogeneous) with examples of each kind, and explanations of how they work. You will also
More informationCHEMICAL KINETICS (RATES OF REACTION)
Kinetics F322 1 CHEMICAL KINETICS (RATES OF REACTION) Introduction Chemical kinetics is concerned with the dynamics of chemical reactions such as the way reactions take place and the rate (speed) of the
More informationCHEM Chemical Kinetics
Chemical Kinetics Catalysts A catalyst is a substance that increases the rate of the reaction but is neither created nor destroyed in the process. Catalysts can be divided into two broad categories. Homogeneous
More informationFACTFILE: GCE CHEMISTRY
FACTFILE: GCE CHEMISTRY 2.9 KINETICS Learning Outcomes Students should be able to: 2.9.1 recall how factors, including concentration, pressure, temperature and catalyst, affect the rate of a chemical reaction;
More information1. (i) 2H 2 O 2 2H 2 O + O 2 ALLOW any correct multiple including fractions IGNORE state symbols 1
1. (i) 2H 2 O 2 2H 2 O + O 2 ALLOW any correct multiple including fractions IGNORE state symbols 1 More crowded particles OR more particles per (unit) volume ALLOW particles are closer together DO NOT
More informationThere is not enough activation energy for the reaction to occur. (Bonds are pretty stable already!)
Study Guide Chemical Kinetics (Chapter 12) AP Chemistry 4 points DUE AT QUIZ (Wednesday., 2/14/18) Topics to be covered on the quiz: chemical kinetics reaction rate instantaneous rate average rate initial
More informationChemical reactions. C2- Topic 5
Chemical reactions C2- Topic 5 What is a chemical reaction? A chemical reaction is a change that takes place when one or more substances (called reactants) form one or more new substances (called products)
More informationTemperature: An increase in temperature increases the rate of reaction.
9 Kinetics I Factors affecting the rate of reaction Temperature: An increase in temperature increases the rate of reaction. Concentration: An increase in the concentration of a solution of reactants increases
More informationWhat does rate of reaction mean?
Junior Science What does rate of reaction mean? It is not how much of a product is made, but instead how quickly a reaction takes place. The speed of a reaction is called the rate of the reaction. What
More informationRate of reaction refers to the amount of reactant used up or product created, per unit time. We can therefore define the rate of a reaction as:
Rates of Reaction Rate of reaction refers to the amount of reactant used up or product created, per unit time. We can therefore define the rate of a reaction as: Rate = change in concentration units: mol
More informationLesmahagow High School CfE Higher Chemistry. Chemical Changes & Structure Controlling the Rate
Lesmahagow High School CfE Higher Chemistry Chemical Changes & Structure Controlling the Rate E a Page 1 of 18 Learning Outcomes Controlling the Rate Circle a face to show how much understanding you have
More informationCHAPTER 9: Rate of Reaction
CHAPTER 9: Rate of Reaction 9.1 Rate of Reaction 9.2 Factors Affecting Rate of Reaction 9.3 Catalysis Learning outcomes: (a) explain and use the terms: rate of reaction, activation energy and catalysis.
More informationC H E M I C N E S C I
C H E M I C A L K I N E T S C I 4. Chemical Kinetics Introduction Average and instantaneous Rate of a reaction Express the rate of a reaction in terms of change in concentration Elementary and Complex
More informationHow many grams of ethylene glycol must be added to 6.00 kg of water to lower its freezing point to C? ETHYLENE GLYCOL:
How many grams of ethylene glycol must be added to 6.00 kg of water to lower its freezing point to -11.0 C? ETHYLENE GLYCOL: 77 KINETICS - the study of the RATE of chemical reactions. Or, the study of
More information6.1 Collision Theory & Rates of Reaction IB SL CHEMISTRY MRS. PAGE
6.1 Collision Theory & Rates of Reaction IB SL CHEMISTRY MRS. PAGE Understandings: Species react as a result of collisions of sufficient energy and proper orientation. The rate of reaction is expressed
More informationReaction Rates and Chemical Equilibrium
Reaction Rates and Chemical Equilibrium 12-1 12.1 Reaction Rates a measure of how fast a reaction occurs. Some reactions are inherently fast and some are slow 12-2 12.2 Collision Theory In order for a
More informationReaction Rates and Chemical Equilibrium
Reaction Rates and Chemical Equilibrium : 12-1 12.1 Reaction Rates : a measure of how fast a reaction occurs. Some reactions are inherently fast and some are slow: 12-2 1 12.2 Collision Theory In order
More information(a) Reaction rates (i) Following the course of a reaction Reactions can be followed by measuring changes in concentration, mass and volume of
(a) Reaction rates (i) Following the course of a reaction Reactions can be followed by measuring changes in concentration, mass and volume of reactants or products. g Measuring a change in mass Measuring
More informationAP Chemistry - Notes - Chapter 12 - Kinetics Page 1 of 7 Chapter 12 outline : Chemical kinetics
AP Chemistry - Notes - Chapter 12 - Kinetics Page 1 of 7 Chapter 12 outline : Chemical kinetics A. Chemical Kinetics - chemistry of reaction rates 1. Reaction Rates a. Reaction rate- the change in concentration
More informationHow fast or slow will a reaction be? How can the reaction rate may be changed?
Part I. 1.1 Introduction to Chemical Kinetics How fast or slow will a reaction be? How can the reaction rate may be changed? *In order to understand how these factors affect reaction rates, you will also
More informationQ1. Methane and oxygen react together to produce carbon dioxide and water.
Chemistry C3 Higher Questions Part 2 Q1. Methane and oxygen react together to produce carbon dioxide and water. The methane gas will not burn in oxygen until a flame is applied, but once lit it continues
More informationChapter 14: Chemical Kinetics
Chapter 14: Chemical Kinetics NOTE THIS CHAPTER IS #2 TOP TOPICS ON AP EXAM!!! NOT ONLY DO YOU NEED TO FOCUS ON THEORY (and lots of MATH) BUT YOU MUST READ THE FIGURES TOO!!! Ch 14.1 ~ Factors that Affect
More informationMgO. progress of reaction
Enthalpy Changes Enthalpy is chemical energy, given the symbol H. We are interested in enthalpy changes resulting from the transfer of energy between chemical substances (the system) and the surroundings
More informationChapter 17. Preview. Lesson Starter Objectives Reaction Mechanisms Collision Theory Activation Energy The Activated Complex Sample Problem A
Preview Lesson Starter Objectives Reaction Mechanisms Collision Theory Activation Energy The Activated Complex Sample Problem A Section 1 The Reaction Process Lesson Starter The reaction H 2 + I 2 2HI
More informationFactors that Affect Reaction Rates
Factors that Affect Reaction Rates Preface: There are 2 kinds of reactions: Homogeneous reactions - all reactants are in the same phase (don't consider products) eg.) 3H 2(g) + N 2(g) 2NH 3(g) Ag + (aq)
More informationALE 1. Chemical Kinetics: Rates of Chemical Reactions
Name Chem 163 Section: Team Number: ALE 1. Chemical Kinetics: Rates of Chemical Reactions (Reference: Sections 16.1 16.2 + parts of 16.5 16.6 Silberberg 5 th edition) How do the surface area, concentration
More informationChapter 16. Rate Laws. The rate law describes the way in which reactant concentration affects reaction rate.
Rate Laws The rate law describes the way in which reactant concentration affects reaction rate. A rate law is the expression that shows how the rate of formation of product depends on the concentration
More informationChemistry 40S Chemical Kinetics (This unit has been adapted from
Chemistry 40S Chemical Kinetics (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 2 Lesson 1: Introduction to Kinetics Goals: Identify variables used to monitor reaction rate. Formulate
More informationChapter 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 informationCHM 111 An introduction to kinetics (r15) 2015 Charles Taylor 1/7
CHM 111 An introduction to kinetics (r15) 2015 Charles Taylor 1/7 Introduction We've talked about chemical reactions many, many times in the past. Up to this point, we've focused on the ingredients you
More informationLecture Presentation. Chapter 14. James F. Kirby Quinnipiac University Hamden, CT. Chemical Kinetics Pearson Education, Inc.
Lecture Presentation Chapter 14 James F. Kirby Quinnipiac University Hamden, CT In chemical kinetics we study the rate (or speed) at which a chemical process occurs. Besides information about the speed
More informationI. Introduction to Reaction Rate
Chemistry 12 Unit 1: Reaction Kinetics 1 I. Introduction to Reaction Rate What is reaction rate? Rate is related to how long it takes for a reaction to go to completion. Measured in terms of: rate of consumption
More informationChapter 14 Chemical Kinetics
Chapter 14 Chemical Kinetics Thermodynamics tells us what can happen and how far towards completion a reaction will proceed. Kinetics tells us how fast the reaction will go. Study of rates of reactions
More informationCHEMISTRY NOTES CHEMICAL KINETICS
CHEMICAL KINETICS Rate of chemical reactions The rate of a reaction tells us how fast the reaction occurs. Let us consider a simple reaction. A + B C + D As the reaction proceeds, the concentration of
More information6.3. Theories of Reaction Rates. Collision Theory. The Effect of Concentration on Reactant Rates
Theories of Reaction Rates 6.3 In section 6.2, you explored the rate law, which defines the relationship between the concentrations of reactants and reaction rate. Why, however, does the rate of a reaction
More information1.4 Enthalpy. What is chemical energy?
1.4 Enthalpy What is chemical energy? Chemical energy is a form of potential energy which is stored in chemical bonds. Chemical bonds are the attractive forces that bind atoms together. As a reaction takes
More informationa) Write the equation for the overall reaction. (Using steps 1 and 2)
Chemistry 12 Reaction Mechanisms Worksheet Name: Date: Block: 1. It is known that compounds called chlorofluorocarbons (C.F.C.s) (eg. CFCl3) will break up in the presence of ultraviolet radiation, such
More informationCHEM Chemical Kinetics. & Transition State Theory
Chemical Kinetics Collision Theory Collision Theory & Transition State Theory The rate of reaction is markedly affected by temperature. k versus T Ae E a k RT Two theories were developed to explain the
More informationFactors that Effect Rate
Factors that Effect Rate Now that we know what has to happen for a reaction to take place (a collision between molecules with the correct orientation and minimum activation energy), let s examine what
More informationCFC: chlorofluorocarbons
The rate of reaction is markedly affected by temperature. Chemical Kinetics & k versus T Two theories were developed to explain the temperature effects. 1. 2. 2 UV radiation strikes a CFC molecule causing
More informationCollision Theory. and I 2
Collision Theory To explain why chemical reactions occur, chemists have proposed a model, known as collision theory, which states that molecules must collide in order to react. These collisions can involve
More informationCh 13 Rates of Reaction (Chemical Kinetics)
Ch 13 Rates of Reaction (Chemical Kinetics) Reaction Rates and Kinetics - The reaction rate is how fast reactants are converted to products. - Chemical kinetics is the study of reaction rates. Kinetics
More informationChemical Kinetics. Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of reactions:
Chemical Kinetics Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of reactions: reactant concentration temperature action of catalysts surface
More informationUnderstanding Equations
Chemical Reactions Chemical reaction: a process of chemically changing both the physical and chemical properties of a substance to a new substance with different physical and chemical properties. Video
More information1.5 Kinetics. Reacting molecules have to collide with enough energy to break the initial bonds, the activation energy.
1.5 Kinetics Collision theory: Reacting molecules have to collide with enough energy to break the initial bonds, the activation energy. Activation energy Activation energy The minimum amount of energy
More informationUnit I: Reaction Kinetics Introduction:
Chemistry 12 Unit I: Reaction Kinetics Introduction: Kinetics Definition: All reactions occur at different rates Examples: Slow Reactions Fast Reactions Chemists need to understand kinetics because sometimes
More informationChapter 14 Chemical Kinetics
Chapter 14 14.1 Factors that Affect Reaction Rates 14.2 Reaction Rates 14.3 Concentration and Rate Laws 14.4 The Change of Concentration with Time 14.5 Temperature and Rate 14.6 Reaction Mechanisms 14.7
More informationName: 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 informationChemistry 12 Worksheet Reaction Mechanisms
Chemistry 12 Worksheet 1-3 - Reaction Mechanisms 1. It is known that compounds called chlorofluorocarbons (C.F.C.s) (eg. CFCl 3 ) will break up in the presence of ultraviolet radiation, such as found in
More information3.2.2 Kinetics. Maxwell Boltzmann distribution. 128 minutes. 128 marks. Page 1 of 16
3.2.2 Kinetics Maxwell Boltzmann distribution 128 minutes 128 marks Page 1 of 16 Q1. The diagram shows the Maxwell Boltzmann distribution for a sample of gas at a fixed temperature. E a is the activation
More informationChapter 14: Chemical Kinetics II. Chem 102 Dr. Eloranta
Chapter 14: Chemical Kinetics II Chem 102 Dr. Eloranta Rate Laws If you are familiar with calculus Experiments would allow you to determine the reaction order and rate constant, but what if you wanted
More informationQ1. (a) State what is meant by the term activation energy of a reaction. (1)
Q1. (a) State what is meant by the term activation energy of a reaction. (c) State in general terms how a catalyst increases the rate of a chemical reaction. The curve below shows the Maxwell Boltzmann
More informationChemistry 30: Reaction Kinetics. Practice Problems
Name: Period: Chemistry 30: Reaction Kinetics Practice Problems Date: Measuring Reaction Rates 1. A chemist wishes to determine the rate of reaction of zinc with hydrochloric acid. The equation for the
More informationOutline: Kinetics. Reaction Rates. Rate Laws. Integrated Rate Laws. Half-life. Arrhenius Equation How rate constant changes with T.
Chemical Kinetics Kinetics Studies the rate at which a chemical process occurs. Besides information about the speed at which reactions occur, kinetics also sheds light on the reaction mechanism (exactly
More information( ) Natural Sciences Department. Chemical Reactions
Chemical Reactions Why do atoms cluster? The attraction which keeps atoms united one to each other to form a molecule is called chemical bond. The atoms place themselves in the molecule so that the energy
More informationKinetics CHAPTER IN THIS CHAPTER
CHAPTER 14 Kinetics IN THIS CHAPTER Summary: Thermodynamics often can be used to predict whether a reaction will occur spontaneously, but it gives very little information about the speed at which a reaction
More informationAtomic Masses and Molecular Formulas *
OpenStax-CNX module: m44278 1 Atomic Masses and Molecular Formulas * John S. Hutchinson This work is produced by OpenStax-CNX and licensed under the Creative Commons Attribution License 3.0 1 Introduction
More informationMITOCW watch?v=ed_xr1bzuqs
MITOCW watch?v=ed_xr1bzuqs The following content is provided under a Creative Commons license. Your support will help MIT OpenCourseWare continue to offer high quality educational resources for free. To
More information6.4 and 6.5 FACTORS AFFECTING REACTION RATES. Factors Affecting the Rate of a Homogenous or Heterogeneous Reaction:
6.4 and 6.5 FACTORS AFFECTING REACTION RATES Homogeneous reactions Heterogeneous reactions Factors Affecting the Rate of a Homogenous or Heterogeneous Reaction: 1. Temperature Maxwell-Boltzmann Distribution
More informationUnit 4, Lesson 03: Collision Theory and the Rates of Chemical Reactions Homework
Unit 4, Lesson 03: Collision Theory and the Rates of Chemical Reactions Homework Page 294, Q 13 16 13. Reaction: 2 ClO (g) Cl 2 (g) + O 2 (g) Potential Energy Diagram for Decomposition of ClO (g) activated
More informationChemical 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 informationLecture (3) 1. Reaction Rates. 2 NO 2 (g) 2 NO(g) + O 2 (g) Summary:
Summary: Lecture (3) The expressions of rate of reaction and types of rates; Stoichiometric relationships between the rates of appearance or disappearance of components in a given reaction; Determination
More informationChapter 13 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 informationExampro GCSE Chemistry
Exampro GCSE Chemistry C Chapter 4 Higher Name: Class: Author: Date: Time: 59 Marks: 59 Comments: Page of 0 Q. The picture shows a lump of phosphate rock. Rob Lavinsky, irocks.com CC-BY-SA-3.0 [CC-BY-SA-3.0],
More informationLower Sixth Chemistry. Sample Entrance Examination
Lower Sixth Chemistry Sample Entrance Examination Time allowed: 60 minutes Name: Total : 60 Marks INSTRUCTIONS : Answer all questions Answers should be written in the spaces provided Dictionaries or reference
More informationQ1. (a) Define the term activation energy for a chemical reaction. (2)
Q1. (a) Define the term activation energy for a chemical reaction. (b) Draw, with labelled axes, a curve to represent the Maxwell Boltzmann distribution of molecular energies in a gas. Label this curve
More informationCollision Theory and Rate of Reaction. Sunday, April 15, 18
Collision Theory and Rate of Reaction Collision Theory System consists of particles in constant motion at speed proportional to temperature of sample Chemical reaction must involve collisions of particles
More informationChemical Kinetics and Equilibrium
Chemical Kinetics and Equilibrium Part 1: Kinetics David A. Katz Department of Chemistry Pima Community College Tucson, AZ USA Chemical Kinetics The study of the rates of chemical reactions and how they
More informationLecture 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 informationCHEMISTRY 2b SUMMARY
CHEMISTRY 2b SUMMARY Items in ITALLICS are HIGHER TIER NLY C2.4.1 RATES F REACTIN Speeding up, or slowing down, chemical reactions is important in everyday life and in industry The rate of a chemical reaction
More informationMechanisms. . CCl2 F + Cl.
Mechanisms 1) Free radical substitution Alkane à halogenoalkane Initiation: Propagation: Termination: Overall: 2) Ozone depletion UV light breaks the C Cl bond releasing chlorine radical CFCl 3 F à. CCl2
More informationSince reactions want to minimize energy you would think that the reaction would be spontaneous like a ball rolling down a hill
Notes 1.1 Exothermic reactions give off heat 120 100 80 60 40 20 0 0 2 4 6 Heat Content Since reactions want to minimize energy you would think that the reaction would be spontaneous like a ball rolling
More information1.3 b) perform calculations, including. 1.4(i) reacting masses (from formulae. candidates answers should reflect the
SUBJECT: CHEMISTRY YEAR: 12 Study PLAN 2017 2018 1 st Term TEACHER: MS. MASOOMA MON TH DATE WEE K Sep 2 nd 1 LEARNING OBJECIIVES PRIOR LEARNING RESOURCES 1 st Term Commences U1: Moles and equation Determine
More informationEquilibrium & Reaction Rate
Equilibrium & Reaction Rate 1. One of the important reactions in coal gasification is the catalytic methanation reaction: CO(g) + H (g) H O(g) + CH 4 (g) H 06 kj a) Predict the direction in which this
More informationIf the order is 0 the value of this term will be 1 no matter what [A] is!
88 CONCNTRATION OF RACTANTS - Usually, the reaction rate increases as you increase the concentration of a reactant. This is true if the order for that reactant is greater than zero! If the order is 0 the
More information(04) WMP/Jan11/CHEM2
Kinetics 4 2 The diagram below shows a Maxwell Boltzmann distribution for a sample of gas at a fixed temperature. E a is the activation energy for the decomposition of this gas. Number of molecules with
More informationc. Methane and oxygen react to form carbon dioxide and water
Name: Date: Period: REVIEW CHAPTERS 10 AND 18 1. Identify the type of each of the following reactions: a. 2Mg + O 2 2 MgO Synthesis b. Fe + CuSO 4 FeSO 4 + Cu Single-Replacement (SR) c. CaCO 3 CaO + CO
More informationKinetics & Equilibrium
Kinetics & Equilibrium Name: Essential Questions How can one explain the structure, properties, and interactions of matter? Learning Objectives Explain Collision Theory Molecules must collide in order
More informationCHEMISTRY 2813/01 How Far, How Fast?
THIS IS A LEGACY SPECIFICATION ADVANCED SUBSIDIARY GCE CHEMISTRY 2813/01 How Far, How Fast? *CUP/T57245* Candidates answer on the question paper A calculator may be used for this paper OCR Supplied Materials:
More informationReaction 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 informationUnit 1. Reaction Kinetics
Unit 1. Reaction Kinetics Given: That butane takes less energy input to burn than a nacho chip; draw the graph of the reaction for both items. Reaction kinetics is the study of the rates and the factors,
More informationChapter 14 Chemical Kinetics
Chapter 14 Chemical Kinetics Learning goals and key skills: Understand the factors that affect the rate of chemical reactions Determine the rate of reaction given time and concentration Relate the rate
More informationExamples of fast and slow reactions
1 of 10 After completing this chapter, you should, at a minimum, be able to do the following. This information can be found in my lecture notes for this and other chapters and also in your text. Correctly
More informationChemistry 12 Unit I Reaction Kinetics Notes
Chemistry 12 Unit I Reaction Kinetics Notes I.1 - Introduction: Reaction kinetics is the study of rates (speeds) of chemical reactions and factors which affect the rates. A fast reaction could be thought
More information1. A. Define the term rate of reaction. The measure of the amount of reactants being converted into products per unit amount of time
Name answer key period IB topic 6 Kinetics 1. A. Define the term rate of reaction. The measure of the amount of reactants being converted into products per unit amount of time b. the reaction between C
More information16+ ENTRANCE EXAMINATION
ST EDWARD S OXFORD 16+ ENTRANCE EXAMINATION For entry in September 2015 CHEMISTRY Time: 1 hour Candidates Name: St Edward's School 1 1. Complete the table below. St Edward's School 2 Element calcium Symbol
More informationQ1. Methane and oxygen react together to produce carbon dioxide and water.
Q1. Methane and oxygen react together to produce carbon dioxide and water. The methane gas will not burn in oxygen until a flame is applied, but once lit it continues to burn. (a) Explain why energy must
More informationA student adds the following volumes of aqueous sodium thiosulfate, dilute hydrochloric acid and distilled water to the conical flask.
1 When aqueous sodium thiosulfate and dilute hydrochloric acid are mixed, a precipitate of insoluble sulfur is produced. This makes the mixture difficult to see through. Na 2 S 2 O 3 (aq) + 2HCl (aq) S(s)
More informationF322: Chains, Energy and Resources Rates and Equilibria
F322: Chains, Energy and Resources 2.3.2 Rates and Equilibria 1. Dilute aqueous hydrogen peroxide, H 2 O 2 (aq), is used to sterilise contact lenses. Dilute H 2 O 2 (aq) slowly decomposes at room temperature
More informationChapter 8: Reaction Rates and Equilibrium
Chapter 8: Reaction Rates and Equilibrium ACTIVATION ENERGY In some reaction mixtures, the average total energy of the molecules is too low at the prevailing temperature for a reaction to take place at
More informationName AP CHEM / / Chapter 12 Outline Chemical Kinetics
Name AP CHEM / / Chapter 12 Outline Chemical Kinetics The area of chemistry that deals with the rate at which reactions occur is called chemical kinetics. One of the goals of chemical kinetics is to understand
More informationUnit 6 Kinetics and Equilibrium.docx
6-1 Unit 6 Kinetics and Equilibrium At the end of this unit, you ll be familiar with the following: Kinetics: Reaction Rate Collision Theory Reaction Mechanism Factors Affecting Rate of Reaction: o Nature
More informationQ1. The gas-phase reaction between hydrogen and chlorine is very slow at room temperature. (g) + Cl 2. (g) 2HCl(g) (2)
Q1. The gas-phase reaction between hydrogen and chlorine is very slow at room temperature. H 2 (g) + Cl 2 (g) 2HCl(g) (a) Define the term activation energy....... Give one reason why the reaction between
More informationKinetics. Chapter 14. Chemical Kinetics
Lecture Presentation Chapter 14 Yonsei University In kinetics we study the rate at which a chemical process occurs. Besides information about the speed at which reactions occur, kinetics also sheds light
More informationCalculating Rates of Substances. Rates of Substances. Ch. 12: Kinetics 12/14/2017. Creative Commons License
Ch. 2: Kinetics An agama lizard basks in the sun. As its body warms, the chemical reactions of its metabolism speed up. Chemistry: OpenStax Creative Commons License Images and tables in this file have
More informationBrown et al, Chemistry, 2nd ed (AUS), Ch. 12:
Kinetics: Contents Brown et al, Chemistry, 2 nd ed (AUS), Ch. 12: Why kinetics? What is kinetics? Factors that Affect Reaction Rates Reaction Rates Concentration and Reaction Rate The Change of Concentration
More informationU N I T T E S T P R A C T I C E
South Pasadena AP Chemistry Name 2 Chemical Kinetics Period Date U N I T T E S T P R A C T I C E Part 1 Multiple Choice You should allocate 30 minutes to finish this portion of the test. No calculator
More informationKinetics is the study of of chemical reactions and the by which they occur.
Kinetics is the study of of chemical reactions and the by which they occur. tells us if a reaction can occur while tells us how quickly the reaction occurs some reactions that are thermodynamically feasible
More information