AP Chemistry 12 Reaction Kinetics III. Name: Date: Block: 1. Catalysts 2. Mechanisms. Catalysts
|
|
|
- Theresa Gray
- 5 years ago
- Views:
Transcription
1 AP Chemistry 12 Reaction Kinetics III Name: Date: Block: 1. Catalysts 2. Mechanisms Catalysts Catalysts provide an alternate reaction pathway in which a different, activated complex can form. Catalysts must be consumed in one step of a reaction mechanism and regenerated in a later step. There are two types of catalysts: Heterogeneous The catalyst is in a phase from the reactants. Typical example: solid catalyst with reactants as either liquids or gases Homogeneous The catalyst is in the phase as the reactants.
2 Mechanisms Elephant s Toothpaste Overall Reaction: Catalyst: Mechanism: Reaction pathways are called. A reaction mechanism is a series of steps that may be added together to give an overall chemical reaction. Cannot be determined by just looking at overall reaction. Deduced through much study and research (up to years) You will not be asked to come up with mechanism from scratch. Some mechanisms are known, however, many are yet to be discovered. Example: (known mechanism) 4 HBr + O 2 2 H 2O + 2 Br 2 Mechanism (determined from lots of research) step 1: HBr + O 2 HOOBr (found to be slow) step 2: HBr + HOOBr 2 HOBr (fast) step 3: 2 HOBr + 2 HBr 2 H 2O + 2 Br 2 (very fast) Each step is called an. ü An is a species that is formed in one step and consumed in a subsequent step and does not appear in the overall reaction. ü Catalysts must be in one step of a reaction mechanism and in a later step. Rate determining step (RDS) - the step in the mechanism. The only way to speed up an overall reaction is to speed up the RDS (eg. by increasing. the concentration of a reactant in the RDS) Speeding up a fast step (not RDS) will have no effect on the overall rate. (eg. adding HOOBr or HOBr has no effect) ü The reactants in the RDS are in the rate law for the reaction.
3 To determining overall reaction, cancel stuff, which is identical on both sides - add up what s left. 1.) A + 2X AX 2 2.) AX 2 + X AX + X 2 3.) AX + A A 2 + X Overall reaction: Intermediates: Catalysts: The following reaction occurs in a 3- step mechanism. Determine the 3 rd step of the mechanism: 2A 4+ + B + 2A 3+ + B 3+ step 1: A 4+ + C 2+ C 3+ + A 3+ step 2: A 4+ + C 3+ C 4+ + A 3+ step 3: Consider the following reaction for the formation of HCl in the presence of light. Determine the 2 nd step of the mechanism. Cl 2 + CHCl 3 HCl + CCl 4 The following is the proposed reaction mechanism: Step 1: Cl 2 Cl + Cl Step 2: Step 3: Cl + CCl 3 CCl 4
4 Returning back to 4 HBr + O 2 2 H 2O + 2 Br 2 step 1: HBr + O 2 HOOBr (found to be slow) step 2: HBr + HOOBr 2 HOBr (fast) step 3: 2 HOBr + 2 HBr 2 H 2O + 2 Br 2 (very fast) PE diagram for the reaction mechanism AC (step 1) AC (step 2) AC (step 3) PE HOOBr HOBr HBr + O2 STEP 1 STEP 2 STEP 3 H2O + Br2 REACTION PROCEEDS Notes: Ø Each bump is a step Ø The higher the bump, (greater Ea) the the step Ø The highest bump (from the reactants level) is for the. Ø AC s at of bumps, intermediates in valleys, products in the valley Ø The Ea for the forward overall reaction is vertical distance from to top of highest bump. Given the following Potential Energy Diagram for a reaction mechanism: 1. This mechanism has steps. PE (KJ) Number each step Ea for overall reaction = kj 3. Step is the RDS 4. Step is the fastest step. 5. The overall reaction is thermic. 6. ΔΗ = kj 7. ΔΗ for reverse rx. = kj Reaction Proceeds 8. Ea (reverse rx.) = kj 9. RDS for reverse reaction is step
5 Draw a Potential Energy Diagram for a reaction mechanism with 2 steps. The first step is fast and the second step is slow. The overall reaction is exothermic. With labeled arrows show the overall Activation Energy (E a ) and the ΔΗ for the forward reaction. PE Reaction Proceeds 1. In the following reaction mechanisms, identify: i. The catalyst ii. The reaction intermediates iii. The overall reaction a) 2 NO à N 2O 2 N 2O 2 + H 2 à N 2O + H 2O N 2O + H 2 à N 2 + H 2O i. ii. iii. b) A + B à C C + D à E + F E + B à D + F i. ii. iii. 2. All catalyzed reaction mechanisms have more than one step. Why must this statement be true? 3. Supposed a catalyzed reaction is occurring in a reaction container. If the catalyst were removed would the reaction stop completely? Explain your answer.
6 4. Consider the following reaction: 2 NO (g) + O 2 (g) 2 NO 2 (g) The rate law is found through experiments to be rate = k[no] 2. A valid mechanism is consistent with the overall equation and the experimentally- determined rate law. Which of the following proposed mechanisms is consistent with the reaction data? Explain your answer. Mechanism 1: (1) NO + O 2 NO 2 + O slow (2) NO + O NO 2 fast Mechanism 2: (1) NO + O 2 D NO 3 fast equilibrium (2) NO 3 + NO 2 NO 2 slow Mechanism 3: (1) 2 NO N 2O 2 slow (2) N 2O 2 + O 2 2 NO 2 fast Complete PE Diagram Worksheet Hebden Workbook Pg. 36 #62, 63
Collision Geometry (comparing alignment)
Collision Geometry (comparing alignment) Hebden # 29-32 consider the rxn: 2 + B 2 2B: E.g. 1) + B B NO RXN E.g. 1collision has alignment (need E for collision to be effective) E.g. 2) B B B + + B B B Reactant
a) 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
Chemistry 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
Reaction Kinetics Multiple Choice
Reaction Kinetics Multiple Choice January 1999 1. Consider the reaction: Ca (s) + 2H 2 O (l) Ca(OH) 2 (aq) + H 2 (g) At a certain temperature, 2.50 g Ca reacts completely in 30.0 seconds. The rate of consumption
a) Write the equation for the overall reaction. (Using steps 1 and 2)
Chemistry 1 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
3. A forward reaction has an activation energy of 50 kj and a H of 100 kj. The PE. diagram, which describes this reaction, is
Kinetics Quiz 4 Potential Energy Diagrams 1. A catalyst increases the rate of a reaction by A. Increasing the concentration of the reactant(s) B. Decreasing the concentration of the reactant(s) C. Increasing
Rates, Temperature and Potential Energy Diagrams Worksheet
SCH4U1 ER10 Name: Date: Rates, Temperature and Potential Energy Diagrams Worksheet Part 1: 1. Use the potential energy diagram shown to the right to answer the following: a. Label the axis. y axis is potential
Chemistry 12 Unit I Reaction Kinetics Study Guide
Chemistry 12 Unit I Reaction Kinetics Study Guide I.1 - Introduction: Reaction kinetics is the study of rates (speeds) of chemical reactions and the factors affect them. Rates of reaction are usually expressed
Answers to Unit 4 Review: Reaction Rates
Answers to Unit 4 Review: Reaction Rates Answers to Multiple Choice 1. c 13. a 25. a 37. c 49. d 2. d 14. a 26. c 38. c 50. d 3. c 15. d 27. c 39. c 51. b 4. d 16. a 28. b 40. c 52. c 5. c 17. b 29. c
Chemistry 12 - Notes on Unit 1 - Reaction Kinetics
Chemistry 12 - Notes on Unit 1 - Reaction Kinetics Expressing Rates rate = quantity of a product formed unit time or rate = quantity of a reactant consumed unit time in general: rate = amount (a reactant
1. Which of the following units could be used to express the reaction rate?
Chemistry 12 Kinetics Practice Test # 2 1. Which of the following units could be used to express the reaction rate? A. ml/s B. ml/g C. g/ml D. ml/mol 2. Consider the reaction: Zn (s) + 2HCl (aq) ZnCl 2(aq)
Since 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
1. Which of the following units could be used to express the reaction rate?
Chemistry 12 Kinetics Practice Test # 2 1. Which of the following units could be used to express the reaction rate? A. ml/s B. ml/g C. g/ml D. ml/mol 2. Consider the reaction: Zn (s) + 2HCl (aq) ZnCl 2(aq)
Unit 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,
1. Draw the PE diagram showing the PE changes that occur during a successful collision of the exothermic reaction:
Ws # 4 Potential Energy Diagrams Worksheet 1. Draw the PE diagram showing the PE changes that occur during a successful collision of the exothermic reaction: H2 + I2 2 HI + 250 KJ The PE of the reactants
Chemistry 12 Review Sheet on Unit 1 -Reaction Kinetics
Chemistry 12 Review Sheet on Unit 1 -Reaction Kinetics 1. Looking at the expressions for reaction rate on page 1 SW, write similar expressions with which you could express rates for the following reactions.
Due Date: First day of school if you miss the first day of school, you must send a scanned/pdf copy to Mr. Mejia:
Name: Date: AP Chemistry Summer Assignment Due Date: First day of school if you miss the first day of school, you must send a scanned/pdf copy to Mr. Mejia: jmejia@cboek12.org Assessment: Within the first
Chemistry 12 Provincial Workbook Unit 01: Reaction Kinetics. Multiple Choice Questions
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 1 / 68 Chemistry 1 Provincial Workbook Unit 01: Reaction Kinetics Multiple Choice Questions 1. Which of the following describes what happens
Rate Mechanism Example reaction: 4HBr + O 2 2H 2 O + 2Br 2 all gases rate = k[hbr] [O 2 ]
![Rate Mechanism Example reaction: 4HBr + O 2 2H 2 O + 2Br 2 all gases rate = k[hbr] [O 2 ]](/thumbs/95/126257756.jpg "Rate Mechanism Example reaction: 4HBr + O 2 2H 2 O + 2Br 2 all gases rate = k[hbr] [O 2 ]")
Name Date Rate Mechanism Example reaction: 4HBr + O 2 2H 2 O + 2Br 2 all gases rate = k[hbr] [O 2 ] What is the likelihood that all 5 of those molecules will collide simultaneously? Balanced chemical equations
1. Consider the reaction X + Y ==> Z. Which rate law corresponds to a zero order reaction?
AP Chemistry Kinetics Review Sheet (CQ) 1. Consider the reaction X + Y ==> Z. Which rate law corresponds to a zero order reaction? 2. Consider the reaction X + Y ==> Z. Which rate law corresponds to a
KINETICS STUDY GUIDE- Written INTRODUCTION
Written Kinetics KINETICS STUDY GUIDE- Written Section: What follows is a comprehensive guide to the written component of the Chemistry 12 Provincial exam for the Unit. The questions below are from previous
I.1 REACTION KINETICS
I.1 REACTION KINETICS KEY QUESTION: Why do reactions occur and how do you control them? REACTION KINETICS is the study of the REACTION RATES Express REACTION RATE as Example 1: The rate of a reaction is
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
UNIT 15 - Reaction Energy & Reaction Kinetics. I. Thermochemistry: study of heat in chemical reactions and phase changes
I. Thermochemistry: study of heat in chemical reactions and phase changes II. A. Heat equation (change in temperature): Q = m. C. p T 1. Q = heat (unit is Joules) 2. m = mass (unit is grams) 3. C p = specific
Factors 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)
Gases have important properties that distinguish them from solids and liquids:
Kinetic molecular theory Gases have important properties that distinguish them from solids and liquids: Gases diffuse to occupy available space. For example, the molecules responsible for the scent of
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
4. Which of the following equations represents an endothermic reaction?
Chem 12 Practice Kinetics Test 1. Consider the following reaction mechanism: step 1: M + X MX step 2: MX + A D + X The chemical species MX is a(n) A. catalyst B. inhibitor C. final product D. reaction
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
Energy Diagram Endothermic Reaction Draw the energy diagram for exothermic and endothermic reactions. Label each part.
CP Chapter 18 Notes A Model for Reaction Rates Expressing Reaction Rates Average Rate = Δquantity Δtime The amount of increase or decrease depends on their mole ratios Units = or mol/ls Expressing Reaction
Chemistry 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. Rates of reaction are usually
Name Unit 10 Practice Test
1. Increasing the temperature increases the rate of a reaction by A) lowering the activation energy B) increasing the activation energy C) lowering the frequency of effective collisions between reacting
10.02 PE Diagrams. 1. Given the equation and potential energy diagram representing a reaction:
10.02 PE Diagrams 1. Given the equation and potential energy diagram representing a reaction: 3. Given the potential energy diagram and equation representing the reaction between substances A and D : If
Unit 1 ~ Learning Guide Name:
Unit 1 ~ Learning Guide Name: Instructions: Using a pencil, complete the following notes as you work through the related lessons. Show ALL work as is explained in the lessons. You are required to have
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
(Ws # 5) Worksheet Mechanisms: Key
(Ws # 5) Worksheet 1.9-1.12 Mechanisms: Key 1. OCl - + H2O HOCl + OH - HOCl + I - HOI + Cl - HOI + OH - H2O + OI - i) The net chemical equation is: OCl - + I - + Cl - +OI - ii) The reaction intermediates
1. The Haber- Bosch Process 2. K eq
Chemistry 12 Equilibrium III Name: Date: Block: 1. The Haber- Bosch Process 2. K eq The Haber- Bosch Process Almost all of the world s ammonia is produced via the Haber- Bosch process and almost all of
14.1 Factors That Affect Reaction Rates
14.1 Factors That Affect Reaction Rates 1) 2) 3) 4) 14.2 Reaction Rates How does increasing the partial pressures of the reactive components of a gaseous mixture affect the rate at which the compounds
Concentration 0. 5 M solutions 1. 0 M solutions. Rates Fast Slow. Which factor would account for the faster reaction rate in Experiment 1?
72. Consider the following experimental results: Experiment 1 Experiment 2 2+ - - 4 2 2 4 aq Reactants Fe ( aq) + MnO4 ( aq) MnO ( aq) + H C O ( ) Temperature 20 C 40 C Concentration 0. 5 M solutions 1.
Equilibrium & 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
Chemistry 12 Reaction Kinetics I. Name: Date: Block: 1. Calculating Rates 2. Measuring Rates 3. Factors Affecting Rates
Chemistry 12 Reaction Kinetics I Name: Date: Block: 1. Calculating Rates 2. Measuring Rates 3. Factors Affecting Rates Monitoring and Calculating Reaction Rates Reaction Rate = Time units: Rate Units:
HC- Kinetics and Thermodynamics Test Review Stations
HC- Kinetics and Thermodynamics Test Review Stations Station 1- Collision Theory and Factors Affecting Reaction Rate 1. Explain the collision theory of reactions. 2. Fill out the following table to review
Chemistry 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
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
Chapter 14 - Chemical Kinetics. Reaction Rates Rate Laws Rate Constants Effect of Concentration on Reaction Rate
Chapter 14 - Chemical Kinetics Reaction Rates Rate Laws Rate Constants Effect of Concentration on Reaction Rate Kinetics The study of the factors that affect the speed of a reaction and the mechanism by
How 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
Unit 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
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
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,
CHEMICAL 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
7.4 Potential Energy Diagrams
Name: Date: Chemistry ~ Ms. Hart Class: Anions or Cations Remember: 7.4 Potential Energy Diagrams Chemical reactions can react in both the and directions All chemical reactions need Reactions can either
Chemical Equilibrium. Chapter 8
Chemical Equilibrium Chapter 8 Equilibrium is a state in which there are no observable changes as time goes by. Chemical equilibrium is achieved when: the rates of the forward and reverse reactions are
Which of the following units could be used to express reaction rate? Reaction Kinetics Monster Review
Chemistry 12 Reaction Kinetics Monster Review 1. Which of the following units could be used to express reaction rate? A. ml s B. ml g C. g ml D. ml mol 2. Consider the reaction: Zn( s) + 2HCl( aq) ZnCl2(
Chapter 15 Chemical Equilibrium
Equilibrium To be in equilibrium is to be in a state of balance: Chapter 15 Chemical Equilibrium - Static Equilibrium (nothing happens; e.g. a tug of war). - Dynamic Equilibrium (lots of things happen,
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
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
Mr. Bracken. Kinetics: Multiple Choice Review Questions
Mr. Bracken AP Chemistry Name Period Kinetics: Multiple Choice Review Questions 1. In the rate law, Rate = k[no] 2 [O 2 ], the reaction is order for NO, order for O 2, and order overall. (a) second; first;
Chapter 16. Rate Laws. The rate law describes the way in which reactant concentration affects reaction rate.
Rate Laws The rate law describes the way in which reactant concentration affects reaction rate. A rate law is the expression that shows how the rate of formation of product depends on the concentration
Unit 13 Kinetics & Equilibrium Page 1 of 14 Chemistry Kinetics, Entropy, Equilibrium, LeChatelier s Principle, K, Unit 13 Quiz: Unit 13 Test:
Unit 13 Kinetics & Equilibrium Page 1 of 14 Chemistry Kinetics, Entropy, Equilibrium, LeChatelier s Principle, K, Unit 13 Quiz: Unit 13 Test: Final Project: VOCABULARY: 1 Chemical equilibrium 2 equilibrium
Chemistry 1B, Fall 2012 Lecture 23
Chemistry 1B Fall 01 [more] Chemical Kinetics 1 kinetics and mechanism of reaction NO (g) + CO(g) ô NO(g) + CO (g) at T< 500K if the reaction was a collision between a NO molecule and a CO molecule one
Worksheet 21 - Le Chatelier's Principle
Worksheet 21 - Le Chatelier's Principle Le Chatelier's Principle states that if a stress is applied to a system at equilibrium, the system will adjust, to partially offset the stress and will reach a new
Unit 2: Chemical Kinetics Chemistry 30
Practice Questions Section 3.2 Factors Influencing Reaction Rate - Activation Energy 1. Answer the following questions based on the potential energy diagram shown here: a. Does the graph represent an endothermic
Chapter 14. Chemical Kinetics
Chapter 14. Chemical Kinetics Common Student Misconceptions It is possible for mathematics to get in the way of some students understanding of the chemistry of this chapter. Students often assume that
In a forward reaction, the reactants collide to produce products and it goes from left to
Worksheet #1 Approaching Equilibrium Read unit II your textbook. Answer all of the questions. Do not start the questions until you have completed the reading. Be prepared to discuss your answers next period.
Welcome to Navigate Powered by NIDES Chemistry 12! Please note that the First Assignment is a requirement to be registered in the course.
Welcome to Navigate Powered by NIDES Chemistry 12! Please note that the First Assignment is a requirement to be registered in the course. Legal last name: First name: Student Email: Cell Phone #: Other
Chapter 14 Chemical Kinetics
Chapter 14 Chemical Kinetics Thermodynamics tells us what can happen and how far towards completion a reaction will proceed. Kinetics tells us how fast the reaction will go. Study of rates of reactions
Chemistry 1B, Fall 2016 Topic 23
Chemistry 1B Fall 016 [more] Chemical Kinetics 1 goals for topic 3 kinetics and mechanism of chemical reaction energy profile and reaction coordinate activation energy and temperature dependence of rate
Practice E4 Mechanisms Name Per
Practice E4 Mechanisms Name Per 1. In a study of nitrosyl halides, a chemist proposes the following mechanism for the synthesis of nitrosyl bromide, NOBr, from nitrogen monoxide and bromine vapor. 20 kj
1. Opp. Khuda Baksh Library, Ashok Rajpath, Patna House no. 5A/65, Opp. Mahual Kothi, Alpana Market, Patna
1. Which of the following expressions does NOT represent a proper expression for the rate of this reaction? 2A + 3B F + 2G a) (- [A)/( t) b) (- [B)/(3 t) c) ( [F)/( t) d) ( [G)/(2 t) e) (- [A)/(2 t) 2.
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
Chemical Kinetics. What quantities do we study regarding chemical reactions? 15 Chemical Kinetics
Chemical Kinetics Chemical kinetics: the study of reaction rate, a quantity conditions affecting it, the molecular events during a chemical reaction (mechanism), and presence of other components (catalysis).
Collision 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
In order for two molecules to react, they must with each other. When they collide they transfer among themselves.
Chemistry 12 Reaction Kinetics II Name: Date: Block: 1. Collision Theory 2. Activation Energy 3. Potential Energy Diagrams Collision Theory (Kinetic Molecular Theory) In order for two molecules to react,
Semester 2 Midterm Review (Bluffer s Guide) *Adapted from Paul Groves [South Pasadena HS]
![Semester 2 Midterm Review (Bluffer s Guide) *Adapted from Paul Groves [South Pasadena HS]](/thumbs/82/86175881.jpg "Semester 2 Midterm Review (Bluffer s Guide) *Adapted from Paul Groves [South Pasadena HS]")
Semester 2 Midterm Review (Bluffer s Guide) *Adapted from Paul Groves [South Pasadena HS] Unit 5: Kinetics How to talk about Reaction Rate rate = Δ[chemical]/Δtime - Common Units: M/s, mol L - s rate of
a) Write the expression for the equilibrium constant, K eq
Chemistry 12 K eq Calculations Worksheet Name: Date: Block: 1. Given the equilibrium equation below: A 2(g) + B 2(g) 2AB (g) If, at equilibrium, the concentrations are as follows: [A 2] = 3.45 M, [B 2]
UNIT I PPT #2 Collision Theory KEY.notebook. September 28, 2010 UNIT I COLLISION THEORY COLLISION THEORY COLLISION THEORY.
UNIT I Collision Theory COLLISION THEORY explains rates on the molecular level Basic Premise: before molecules can react, they must collide http://www.chem.iastate.edu/group/greenbowe/section s/projectfolder/animations/no+o3singlerxn.html
(g) burns according to this reaction? D) CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(l)
Name: 7171-1 - Page 1 1) In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is defined as the A) heat of reaction B) ionization
CHEM 102 Winter 10 Exam 2(a)
CHEM 102 Winter 10 Exam 2(a) On the answer sheet (scantron) write your Name, Student ID Number, and Recitation Section Number. Choose the best (most correct) answer for each question AND ENTER IT ON YOUR
B. The rate will increase by a factor of twelve. C. The rate will increase by a factor of twenty-four. D. The rate will decrease by a factor of six.
1. If O 2 (g) disappears at a rate of 0.250 M/s at a particular moment in the reaction below, what is the rate of appearance of H 2 O(g) at the same time? C 3 H 8 (g) + 5 O 2 (g) 3 CO 2 (g) + 4 H 2 O(g)
Chemistry 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
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
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
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:
Chemistry 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
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
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
Regents Review Kinetics & Equilibrium Worksheet Mr. Beauchamp
Regents Review Kinetics & Equilibrium Worksheet Mr. Beauchamp 1. Which event must always occur for a chemical r eaction to take place? A. formation of a precipitate B. formation of a gas C. effective collisions
Unit 13: Rates and Equilibrium- Guided Notes
Name: Period: What is a Chemical Reaction and how do they occur? Unit 13: Rates and Equilibrium- Guided Notes A chemical reaction is a process that involves of atoms Law of Conservation of : Mass is neither
33-1. Energy Profiles. Energy Profiles Reactions will:- 1.Break or weaken bonds in reactants then form bonds in products.
Energy Profiles Energy Profiles Reactions will:- 1.Break or weaken bonds in reactants then form bonds in products. 2. Reactants pass over a Potential Energy Barrier on way to Products. Plot: NO 33-1 Energy
Chemistry 6A F2007. Dr. J.A. Mack 11/19/07. Chemical Kinetics measure the rate of appearance of products or the rate of disappearance of reactants.
Chemistry 6A F2007 Dr. J.A. Mack Chemical Kinetics measure the rate of appearance of products or the rate of disappearance of reactants. Reactants Products Reactants go away with time. Products appear
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
CHAPTER 17 REVIEW. Reaction Kinetics. Answer the following questions in the space provided. Energy B A. Course of reaction
CHAPTER 17 REVIEW Reaction Kinetics SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Refer to the energy diagram below to answer the following questions. D Energy C d c d
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
Leader: Deborah Course: CHEM 178 Instructor: Bonaccorsi/Vela Date: 2/6/18 + H 2 CHF 3. a. Express the rate law in terms of m, n, and k.
EXAM I REVIEW KEY Leader: Deborah Course: CHEM 178 Instructor: Bonaccorsi/Vela Date: 2/6/18 1. Given the following reaction: CF 4 + H 2 CHF 3 + HF a. Express the rate law in terms of m, n, and k. Rate
10 Reaction rates and equilibrium Answers to practice questions. OCR Chemistry A. number 1 (a) 1: The enthalpy change, H;
1 (a) 1: The enthalpy change, H; 2: The activation energy, E a 1 (b) H is unaffected as it is the difference between the reactants and products E a decreases as a catalyst allows an alternative route of
Unit 9 Kinetics SA Review
1. Base your answer to the following question on the information below. The equilibrium equation below is related to the manufacture of a bleaching solution. In this equation, means that chloride ions
first later later still successful collision ( reaction ) low conc. both high conc. blue high conc. both low conc. red
Collision theory Basic idea (basic premise) http://www.chem.iastate.edu/group/greenbowe/sections/projectfolder/animations/no+o3singlerxn.html - before molecules can react, they must collide. H 2 + I 2
Unit 13: Rates and Equilibrium- Funsheets
Name: Period: Unit 13: Rates and Equilibrium- Funsheets Part A: Reaction Diagrams 1) Answer the following questions based on the potential energy diagram shown here: a. Does the graph represent an endothermic
UNIT II - REVIEW EQUILIBRIA. Part I - Multiple Choice. 1. In which of the following does the entropy decrease?
CHEMISTRY 12 UNIT II - REVIEW EQUILIBRIA Part I - Multiple Choice 1. In which of the following does the entropy decrease? A. NaCl (s) Na + (aq) + Cl (aq) B. 4 NO (g) + 6 H 2 O (g) 4 NH 3 (g) + 5 O 2 (g)
Reaction 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