UNIT 4 CHEMICAL KINETICS
|
|
|
- Solomon Henry
- 5 years ago
- Views:
Transcription
1 Concentration Ankit Gupta Classes UNIT 4 CHEMICAL KINETICS MARK QUESTIONS Q.. In the reaction A B, if the concentration of A is plotted against time, the nature of the curve obtained will be as shown. What is the order of the reaction? Time Ans. First Order Q. 2. What is the effect of temperature on activation energy? Ans. There is no effect of temperature on activation energy. Q. 3. Which will dissolve in water faster, powdered sugar or crystalline sugar and why? Ans. Powdered sugar will dissolve in water faster as it has more surface area. Q. 4. Which reaction will take place faster and why? 500 C C (s) + ½ O 2 (g) CO (g) 000 C C (s) + ½ O 2 (g) CO (g) Ans. The second reaction is faster because increase in temperature increases the number of effective collisions and hence increase in rate.
2 Q. 5. For a reaction A + H 2 O B; r = k [A]. What is its (i) Molecularity Order? Ans. Pseudo unimolecular rection order = 2 MARKS QUESTIONS Q.. A reaction : Reactant Product is represented by : Conc. of reactant (R) [R] 0 Time (t) (i) Predict the order of the reaction. What does the slope of the graph represent? Ans. (i) Zero order Slope = k = d[r] dt Q. 2. For a reaction, the activation energy is zero. What is the value of rate constant at 300 K if K = s at 280 K. Ans. log K2 K = E a T2 T 2.303R TT 2 0 T T 2.303R TT 2 = 2 = 0 K2 K = antilog (0) = or K = K = s Q. 3. The slope of the line in the graph of log K is T for a reaction is 584 K. Calculate E a for the reaction. 2
3 Ans. Slope = Ea 2.303R E a = R Slope = = g/mol 3 MARKS QUESTIONS K Q.. Consider the reaction R P. The change in concentration of A with time is shown in the given plot : y Conc. [R] (i) Ans. (i) Predict the order of the reaction. Derive the expression for the time required for the completion of the reaction. Zero order For the reaction R P r = d[r] = K [R] dt d [R] = K dt On integration [R] = Kt + C Time (t) x When t = 0 [R] = [R] 0 On substitution [R] = Kt [R] 0 [R] = Kt + [R] 0 Kt = [R] 0 [R] t = K {[R] [R]} 0 3
4 Q. 2. Answer the following questions on the basis of the given curve for a first order reaction : A P (i) What is the relation between slope of this line and rate constant? Calculate the rate constant of the above reaction if the slope is s. Ans. (i) Slope = K Slope = s K = Slope = s = s [R 0] log [R] Q. 3. For a certain chemical reaction variation in concentration in [R] VS time plot is given below. For this reaction write : Time (i) What are the units of rate constant? Give the relationship between k and t ½. (iii) What does the slope of the above line indicate? 4
5 Ans. (i) time (s ) K = t 2 (iii) rate constant K of the reaction. Q. 4. Consider the following diagram representing potential energy plot and answer the following questions : (i) What do x and y represent? What does z represent in this diagram? (iii) Is the reaction endothermic or exothermic? Ans. (i) x represents E a for forward reaction. y represents E a for backward reaction. (iii) z represents H, the enthalpy change for the reaction. Exothermic reaction. Q. 5. Consider a plot between k vs T where T is the temperature. On the basis of this plot, answer the following questions : 5
6 y ln k T x (i) What is the slope in this line? What is the intercept of this line on the y-axis? (iii) What is the relation between K and T? Ea Ans. (i) Slope = R Intercept = ln A (iii) ln k T or K = A e Ea/RT Q. 6. Diagram given below shows a plot of potential energy Vs reaction co-ordination for a hypothetical reaction. Write answers to the following from the plot given : (a) Represent reactant, product and activated complex in terms of A, B and C? (b) Is this reaction exothermic or endothermic? (c) What will be the effect of a catalyst on E a of the reaction? 6
7 Ans. (a) A Reactant B Product C Activated Complex (b) (c) Exothermic Catalyst will lower the activation energy for the reaction. Q. 7. The rate of a first order reaction is 0.04 mol/h/s at 0 minutes and 0.03 mol/h/s at 20 minutes. Find the half life period of the reaction. Ans. Rate = K C r = K C r 2 = KC 2 r (0 min) C 0.04 r 20 min C K = t log C C 2 When t = 0 min K = t t ½ = K log = = log 4 3 = 24.4 min. = min 7
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
CHAPTER CHEMICAL KINETICS
161 CHAPTER CHEMICAL KINETICS 1. volume force pressure conc. of reactants Ans: 6. In a reversible reaction the energy of activation of the forward reaction is 50 kcal. The energy of activation for the
CHEMISTRY 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
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
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
14-2 Whether a reaction should proceed (thermodynamics) and how fast (kinetics) it should proceed.
1-2 Whether a reaction should proceed (thermodynamics) and how fast (kinetics) it should proceed. 1-6 The rate of the reaction will slow down as time goes by since the rate is dependent upon the concentration
UNIT-4 CHEMICAL KINETICS CONCEPT
UNIT-4 CHEMICAL KINETICS CONCEPT Thermodynamics helps us to predict the feasibility of chemical reaction by using G as parameter but it cannot tell everything about the rate of reaction. Rate of chemical
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 Kinetics AP Chemistry Lecture Outline
Chemical Kinetics AP Chemistry Lecture Outline Name: Factors that govern rates of reactions. Generally... (1)...as the concentration of reactants increases, rate (2)...as temperature increases, rate (3)...with
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
Chem 116 POGIL Worksheet - Week 6 Kinetics - Part 2
Chem 116 POGIL Worksheet - Week 6 Kinetics - Part 2 Why? A different form of the rate law for a reaction allows us to calculate amounts as a function of time. One variation on this gives us the concept
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
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,
CHEM Chapter 14. Chemical Kinetics (Homework) Ky40
CHEM 1412. Chapter 14. Chemical Kinetics (Homework) Ky40 1. Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2ClO 2 (aq) + 2OH (aq) ClO
LE CHATELIER S PRINCIPLE
LE CHATELIER S PRINCIPLE When a chemical system at equilibrium is subjected to an external stress (disturbed by a change in a property), the system establishes a new equilibrium to minimize the effects
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
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
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
A is the frequency factor (related to the number of collisions)
Chemistry Week 10 Worksheet Notes Oregon State University Ea RT 1. Discuss k e k is the rate is the frequency factor (related to the number of collisions) Ea is the activation energy R is the gas constant
UNIT #10: Reaction Rates Heat/Energy in Chemical Reactions Le Chatlier s Principle Potential Energy Diagrams
UNIT #10: Reaction Rates Heat/Energy in Chemical Reactions Le Chatlier s Principle Potential Energy Diagrams NAME: 1. REACTION RATES a) The speed of a chemical reaction determined by the change in concentration
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
Lecture Presentation. Chapter 14. James F. Kirby Quinnipiac University Hamden, CT. Chemical Kinetics Pearson Education, Inc.
Lecture Presentation Chapter 14 James F. Kirby Quinnipiac University Hamden, CT In chemical kinetics we study the rate (or speed) at which a chemical process occurs. Besides information about the speed
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
Chem 116 POGIL Worksheet - Week 6 Kinetics - Concluded
Chem 116 POGIL Worksheet - Week 6 Kinetics - Concluded Why? The half-life idea is most useful in conjunction with first-order kinetics, which include many chemical reactions and all nuclear decay processes.
The first aspects forms the subject matter of chemical equilibrium. The second aspects forms the subject matter of chemical kinetics.
Chemical Kinetics Introduction In a chemical reaction two important aspects are: (a) How far the reaction will go? and (b) How fast the reaction will occur? The first aspects forms the subject matter of
Chapter 14 Chemical Kinetics
Chapter 14 Chemical Kinetics Learning goals and key skills: Understand the factors that affect the rate of chemical reactions Determine the rate of reaction given time and concentration Relate the rate
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
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
1 The nuclear binding energy is the amount of energy consumed during. 2 An unstable isotope of Ga-73 undergoes radioactive decay to Ga-73
version: master Exam 3 - REVIEW This exam should have 27 questions. The point values are given with each question. Bubble in your answer choices on the bubblehseet provided. Your score is based on what
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
Rates of Chemical Reactions
Rates of Chemical Reactions Jim Birk 12-1 Questions for Consideration 1. What conditions affect reaction rates? 2. How do molecular collisions explain chemical reactions? 3. How do concentration, temperature,
Chemistry 112 Midterm January 30, 2006
1. (35 points) The reaction of A and B to form products is thought to go according to the following mechanism: A + 2B 2C + D k -1 2C 2C 2C + M k 2 k 3 k 4 G H J + M (a) (5) Identify the products in this
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
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
P a g e What is the algebraic sign for enthalpy of solution? A. positive B. negative C. not enough information is given
P a g e 1 Chem 123 Practice Questions for EXAM II Spring 2014 Exam II on Wed 3/12/14 This HAS BEEN updated after Monday s lecture (3/10/14) JUST studying these questions is not sufficient preparation.
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
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
B. Activation Energy: Ea
B. Activation Energy: Ea a) Example reaction: the burning of charcoal in the BBQ C (s) + O 2(g) CO 2 (remember, burning is VERY exothermic) Question: Will charcoal in your BBQ spontaneously catch fire?
CHEMICAL KINETICS Order and molecularity of reactions with examples, zero and first order reaction with examples
CHEMICAL KINETICS Topic-2 Order and molecularity of reactions with examples, zero and first der reaction with examples VERY SHORT ANSWER QUESTIONS 1. What is der of as reaction? Ans: The sum of the powers
Chapter 14: Chemical Kinetics
1. Which one of the following units would not be an acceptable way to express reaction rate? A) M/s B) M min 1 C) L mol 1 s 1 D) mol L 1 s 1 E) mmhg/min 3. For the reaction BrO 3 + 5Br + 6H + 3Br 2 + 3H
RATES & CHEMICAL EQUILIBRIUM Checklist. Exam Questions
RATES & CHEMICAL EQUILIBRIUM Checklist Make sure you can. Explain what reaction rate is and list the factors which affect the rate of chemical reactions Use Collision theory to explain how the various
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:
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
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? 2. Determine the relative reaction rates of
Physical Chemistry Chapter 6 Chemical Kinetics
Physical Chemistry Chapter 6 Chemical Kinetics by Azizul Helmi Sofian Faculty of Chemical & Natural Resources Engineering azizulh@ump.edu.my Chapter Description Aims To define rate laws accordingly To
Kinetics. Consider an irreversible unimolecular reaction k. -d[a]/dt = k[a] Can also describe in terms of appearance of B.
![Kinetics. Consider an irreversible unimolecular reaction k. -d[a]/dt = k[a] Can also describe in terms of appearance of B.](/thumbs/72/67129702.jpg "Kinetics. Consider an irreversible unimolecular reaction k. -d[a]/dt = k[a] Can also describe in terms of appearance of B.")
Kinetic data gives insight into reaction mechanisms kinetic analysis will describe a relationship between concentrations of all chemical species before the rate determining step in a given reaction and
Lecture 2. Review of Basic Concepts
Lecture 2 Review of Basic Concepts Thermochemistry Enthalpy H heat content H Changes with all physical and chemical changes H Standard enthalpy (25 C, 1 atm) (H=O for all elements in their standard forms
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
Log I is plotted vs time in Figure below and slope obtained is 0.72 x 10 4 s -1.
Assignment 4 Chemical Kinetics 1. A reaction is 50% complete in 10 minutes. It is allowed to proceed another 5 minutes. How much of the reaction would be complete at the end of these 15 minutes if the
UNIT 9: KINETICS & EQUILIBRIUM. Essential Question: What mechanisms affect the rates of reactions and equilibrium?
UNIT 9: KINETICS & EQUILIBRIUM Essential Question: What mechanisms affect the rates of reactions and equilibrium? What is Kinetics? Kinetics is the branch of chemistry that explains the rates of chemical
Chemical Kinetics. Reaction Rate. Reaction Rate. Reaction Rate. Reaction Rate. Chapter 13: Chemical Kinetics: Rates of Reactions
Chemical Kinetics The study of speeds of reactions and the nanoscale pathways or rearrangements by which atoms and molecules are transformed to products Chapter 3: Chemical Kinetics: Rates of Reactions
Chemical Kinetics. Reaction Rate. Reaction Rate. Reaction Rate. Reaction Rate. Chemistry: The Molecular Science Moore, Stanitski and Jurs
Chemical Kinetics Chemistry: The Molecular Science Moore, Stanitski and Jurs The study of speeds of reactions and the nanoscale pathways or rearrangements by which atoms and molecules are transformed to
İTÜ GELİŞTİRME VAKFI ÖZEL EKREM ELGİNKAN LİSESİ. Term Lesson Unit Subject Date. 2nd Chemistry Unit Review
İTÜ GELİŞTİRME VAKFI ÖZEL EKREM ELGİNKAN LİSESİ Term Lesson Unit Subject Date 2nd Chemistry Unit 5-6-7 Review 25.04-03.05 2015 Name- Surname Class: 10-IB Number: 1. What is the function of iron in the
Energy Changes, Reaction Rates and Equilibrium. Thermodynamics: study of energy, work and heat. Kinetic energy: energy of motion
Energy Changes, Reaction Rates and Equilibrium Thermodynamics: study of energy, work and heat Kinetic energy: energy of motion Potential energy: energy of position, stored energy Chemical reactions involve
KINETICS CHEMICAL CHEMIC. Unit. I. Multiple Choice Questions (Type-I)
Unit 4 CHEMICAL CHEMIC KINETICS I. Multiple Choice Questions (Type-I) 1. The role of a catalyst is to change. gibbs energy of reaction. enthalpy of reaction. activation energy of reaction. equilibrium
Rates and Temperature
Rates and Temperature N Goalby Chemrevise.org Activation Energy Molecules will only react if they collide with enough energy to break the relevant bonds in one or either of the reactant molecules. This
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,
3.2.2 Kinetics. Effect of Concentration. 135 minutes. 134 marks. Page 1 of 13
3.. Kinetics Effect of Concentration 35 minutes 34 marks Page of 3 M. (a) Activation energy;- The minimum energy needed for a reaction to occur / start () Catalyst effect:- Alternative route (or more molecules
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
Practice test Chapter 12 and 13
Practice test Chapter 12 and 13 1. Which of the following pure liquids is the best solvent for carbon disulfide? A) C6H6(l) B) NH3(l) C) CH3OH(l) D) H2O(l) E) HBr(l) 2. How does the solubility of a gas
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
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
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
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
Yes. Yes. Yes. Experimental data: the concentration of a reactant or product measured as a function of time. Graph of conc. vs.
Experimental data: the concentration of a reactant or product measured as a function of time Graph of conc. vs. time Is graph a straigh t line? No Graph of ln[conc.] vs. time Yes System is zero order Is
Bond Enthalpy and Activation Energy
Bond Enthalpy and Activation Energy Energy of a Chemical Reaction ΔH = ΔH (bonds broken) - ΔH (bonds formed) Add up all the energies of the broken bonds Add up all the energies of the bonds that are reformed
Chemistry 102 Chapter 14 CHEMICAL KINETICS. The study of the Rates of Chemical Reactions: how fast do chemical reactions proceed to form products
CHEMICAL KINETICS Chemical Kinetics: The study of the Rates of Chemical Reactions: how fast do chemical reactions proceed to form products The study of Reaction Mechanisms: the steps involved in the change
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
REACTION KINETICS. Catalysts substances that increase the rates of chemical reactions without being used up. e.g. enzymes.
REACTION KINETICS Study of reaction rates Why? Rates of chemical reactions are primarily controlled by 5 factors: the chemical nature of the reactants 2 the ability of the reactants to come in contact
Enter all MC answers into the Response System
Kinetics Unit Test AP Chemistry Please Do Not Write On MC Exam Enter all MC answers into the Response System Base your answers to questions 1 and 2 on the possible rate laws below for the reaction: A +
KEY for CHEM 116 EXAM #2 PRACTICE
Circle the correct answers ( points each) KEY for CHEM 6 EXAM # PRACTICE. If the half-life of a reaction depends on the concentration of the reactant, then the reaction cannot be order. a. second b. zero
Questions 1-3 relate to the following reaction: 1. The rate law for decomposition of N2O5(g) in the reaction above. B. is rate = k[n2o5] 2
![Questions 1-3 relate to the following reaction: 1. The rate law for decomposition of N2O5(g) in the reaction above. B. is rate = k[n2o5] 2](/thumbs/91/106996700.jpg "Questions 1-3 relate to the following reaction: 1. The rate law for decomposition of N2O5(g) in the reaction above. B. is rate = k[n2o5] 2")
Questions 1-3 relate to the following reaction: 2N2O5(g) 4NO2(g) + O2(g) 1. The rate law for decomposition of N2O5(g) in the reaction above A. is rate = k[n2o5] B. is rate = k[n2o5] 2 C. is rate = [NO2]
Chemical Equilibrium
Chemical Equilibrium Forward Rxn: A + B C + D Reverse Rxn: A + B C + D Written as: A + B C + D OR A + B C + D A reversible reaction has both an endothermic rxn and an exothermic rxn Reactants Exothermic
What is the volume of the unit cell of Ni in ml?
P a g e 1 Chem 123 Practice Questions for EXAM II Fall 2014 Exam II on Mon 10/13/14 This HAS BEEN updated after Wed s lecture (10/8/14) JUST studying these questions is not sufficient preparation. There
4)Instantaneous rate: It is defined as the rate of a reaction at a specific instant.
I) DEFINITIONS: CHEMICAL KINETICS F.Y.B.Sc 1) Chemical kinetics: It is a branch in physical chemistry which deals with the study of rate of a chemical reaction, the factor affecting their rates and the
AP * Chemistry. Kinetics: Integrated Rate Law & Determining Ea. René McCormick
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
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Chemistry 213 Exam I - A Spring 2010 Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) At elevated temperatures, methylisonitrile (CH3NC) isomerizes
Examples of fast and slow reactions
1 of 10 After completing this chapter, you should, at a minimum, be able to do the following. This information can be found in my lecture notes for this and other chapters and also in your text. Correctly
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
Homework 07. Kinetics
HW07 - Kine!cs Started: Mar at 10:56am Quiz Instruc!ons Homework 07 Kinetics Question 1 Consider the reaction: O (g) 3O (g) rate = k[o ] [O ] 3 3 What is the overall order of the reaction and the order
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
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
Chapter 14, Chemical Kinetics
Last wee we covered the following material: Review Vapor Pressure with two volatile components Chapter 14, Chemical Kinetics (continued) Quizzes next wee will be on Chap 14 through section 14.5. 13.6 Colloids
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
Assessment Schedule 2016 Chemistry: Demonstrate understanding of chemical reactivity (91166)
NCEA Level 2 Chemistry (91166) 2016 page 1 of 6 Assessment Schedule 2016 Chemistry: Demonstrate understanding of chemical reactivity (91166) Evidence Statement Q Evidence Achievement Merit Excellence ONE
Kinetics Worksheet. Version A
1. Which event must always occur for a chemical reaction to take place? (A) formation of a precipitate (B) formation of a gas (C) effective collisions between reacting particles (D) addition of a catalyst
(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
Use your time wisely. Do not get stuck on one question. WORK MUST BE SHOWN CAREFULLY, WITH UNITS AT EVERY STEP OF SETUP.
Spring 2014 CCBC-Catonsville (Wed 3/12/14) Use your time wisely. Do not get stuck on one question. WORK MUST BE SHOWN CAREFULLY, WITH UNITS AT EVERY STEP OF SETUP. PAGE TOTAL SCORE POSSIBLE YOUR SCORE
7.1 Dynamic Equilibrium
7.1 Dynamic 7.1.1 - Outline the characteristics of chemical and physical systems in a state of equilibrium Open system When a reaction occurs in an unsealed container Closed system When a reaction occurs
Chemical Kinetics 1. Reading: Ch 13, sections1-2 Homework: Chapter 13: 3, 5, 25*, 27, 29*, 31*
Chemical Kinetics 1 Reading: Ch 13, sections1-2 Homework: Chapter 13: 3, 5, 25*, 27, 29*, 31* * = important homework question Factors that Affect Reaction Rates General Discussion: Fundamentally speaking,
12.1 Reaction Rates. Reaction rate is defined as the change in concentration of a reactant or product per time. 2NO2 2NO + O2. In terms of reactants:
Kinetics Unit 5 12.1 Reaction Rates Reaction rate is defined as the change in concentration of a reactant or product per time. 2NO2 2NO + O2 In terms of reactants: The rate will be negative because the
CHEMICAL KINETICS. Collision theory and concepts, activation energy and its importance VERY SHORT ANSWER QUESTIONS
Topic-3 CHEMICAL KINETICS Collision theory and concepts, activation energy and its importance 1. What is law of mass action? VERY SHORT ANSWER QUESTIONS This law relates rate of reaction with active mass
Unit - 4 CHEMICAL KINETICS VSA QUESTIONS (1 - MARK QUESTIONS) (aq) as product for the reaction : 5 Br (aq) + Br(aq) + 6H + (aq) 3 Br 2
Unit - 4 CHEMICAL KINETICS VSA QUESTIONS (1 - MARK QUESTIONS) 1. Define the term rate of reaction. 2. Mention the units of rate of reaction. 3. Express the rate of reaction in terms of Br (aq) as reactant
4) What is the order of the reaction with respect to ClO2? 4) A) 2 B) 1 C) 4 D) 0 E) 3
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 1) 2NO2 2NO
Chemical Reaction (IGCSE Chemistry Syllabus )
Chemical Reaction (IGCSE Chemistry Syllabus 2016-2018) Collision Theory o Collision of particles are needed for a chemical reaction to take place o Successful collision: particles have enough activation
3. Increased surface area (1) more collisions (1) 2
3. Increased surface area (1) more collisions (1) 2 Mill Hill High School 1 [9] (c) (i) 2H 2 O 2 2H 2 O + O 2 1 (ii) Speeds up (alters the rate of) a chemical reaction 1 Remains unchanged (or not used
1. Introduction to Chemical Kinetics
1. Introduction to Chemical Kinetics objectives of chemical kinetics 1) Determine empirical rate laws H 2 + I 2 2HI How does the concentration of H 2, I 2, and HI change with time? 2) Determine the mechanism
Name Practice Questions Date Kinetics
Name Practice Questions Date Kinetics 1. An experiment was conducted to determine the rate law of the reaction 2 A + 2 B C + D. The data collected is shown below. Base your answers to questions 8 and 9
Wksht Rate Laws
Wksht 1.1 - Rate Laws Iowa State University Leader: Deborah Course: CHEM 178 Instructor: Bonaccorsi/Vela Date: 1/16/18 1. Describe the difference between average rate and instantaneous rate. Average rate-
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