1. 13-1 CHEM 102, Spring 2014, LA TECH Instructor: Dr. Upali Siriwardane e-mail: upali@latech.edu Office: CTH 311 Phone 257-4941 Office Hours: M,Tu, W,Th,F 9:00-11:00 am ; Test Dates : 9:30-10:45 am., DAVH 209 Chemistry 102(60) Summer 2014 July 21, 2014 (Test 1): Chapter 13 July 28, 2014 (Test 2): Chapter 14 August 5, 2014 (Test 3): Chapter 15 &16 August 13, 2014 (Test 4) Chapter 17 August 14, 2014 (Make-up test) comprehensive: Chapters 13-17

2. 13-2 CHEM 102, Spring 2014, LA TECH Chapter 13. Chemical Kinetics 13.1 Catching Lizards 563 13.2 The Rate of a Chemical Reaction 564 13.3 The Rate Law: The Effect of Concentration on Reaction Rate 569 13.4 The Integrated Rate Law: The Dependence of Concentration on Time 573 13.5 The Effect of Temperature on Reaction Rate 581 13.6 Reaction Mechanisms 588 13.7 Catalysis 593

3. 13-3 CHEM 102, Spring 2014, LA TECH Why Study Rates of Reactions? 1) Rates show us how fast/slow a reaction would take place. 2) We need make some reactions go faster. 3) Some reactions needed to be slowed down. 4) We need the conceptual back ground of the “factors” that would change the rate of a reaction 5) In this chapter we will go through models and the theories dealing with reaction rates (Chemical Kinetics)

4. 13-4 CHEM 102, Spring 2014, LA TECH How do you measure rates? How do you measure rates? Rates are related to the time it required to decay Rates are related to the time it required to decay reactants or form products. The rate reaction = change in concentration of The rate reaction = change in concentration of reactants/products per unit time Average rate Average rate rate of reaction = –  [reactant]/  t Instantaneous rate Instantaneous rate rate of reaction = – d[reactant]/dt H 2 + I 2 --> 2 HI

5. 13-5 CHEM 102, Spring 2014, LA TECH Reaction of cis-platin with Water Substitution reaction

6. 13-6 CHEM 102, Spring 2014, LA TECH Disappearance of Color Intensity of Color is proportional to amount of reactant

7. 13-7 CHEM 102, Spring 2014, LA TECH

8. 13-8 CHEM 102, Spring 2014, LA TECH Rate of Appearance & Disappearance is different from Reaction Rates 2 N 2 O 5 (g) -----> 4 NO 2 (g) + O 2 (g) Disappearance is based on reactants rate = -(  [N 2 O 5 ]/  t Appearance is based on products rate =  [NO 2 ]/  t rate =  [O 2 ]/  t Converting rates of Appearance and disappearance. rate = (  [NO 2 ]/  t = - 4/2  [N 2 O 5 ]/  t  [O 2 ]/  t = - 1/2  [N 2 O 5 ]/  t

9. 13-9 CHEM 102, Spring 2014, LA TECH Measuring Reaction Rate a A --> b B Based on reactants rate = -(1/a)  [A]/  t Based on products rate = +(1/b)  [B]/  t  [A]= [A] f - [A] I Change in A  t= t f - t i Change in t

10. 13-10 CHEM 102, Spring 2014, LA TECH 1) What is the rate of a chemical reaction? (Describe in your own words and then in equation) a A ----> b B + c C a A ----> b B + c C

11. 13-11 CHEM 102, Spring 2014, LA TECH 2) Answer the following Given the chemical reaction: 2 N 2 O 5 ----> 4 NO 2 + O 2 a) What’s the rate of disappearance ( or decomposition) N 2 O 5 ? (Equation) b) What are the rates of appearance of NO 2 and O 2 ? (Equations)

12. 13-12 CHEM 102, Spring 2014, LA TECH 2) Answer the following Given the chemical reaction: 2 N 2 O 5 ----> 4 NO 2 + O 2 c) What are the rates of reaction based on N 2 O 5, NO 2, and O 2 ? (Equations) d) Are the rates of decomposition based on N 2 O 5, and formation based on, NO 2, and O 2 equal? (Explanation)

13. 13-13 CHEM 102, Spring 2014, LA TECH 2) Answer the following Given the chemical reaction: 2 N 2 O 5 ----> 4 NO 2 + O 2 e) Are the rate of reaction based on N 2 O 5, NO 2, and O 2 equal? (Equations and explanation)

14. 13-14 CHEM 102, Spring 2014, LA TECH 2) Answer the following Given the chemical reaction: 2 N 2 O 5 ----> 4 NO 2 + O 2 e) Are the rate of reaction based on N 2 O 5, NO 2, and O 2 equal? (Equations and explanation)

15. 13-15 CHEM 102, Spring 2014, LA TECH 3) What are the differences between average and instantaneous reaction rates? Refer to graph in new concepts. 4) Why is instantaneous rates of N 2 O 5 and NO 2 are negative and positive respectively?

16. 13-16 CHEM 102, Spring 2014, LA TECH 3) What are the differences between average and instantaneous reaction rates? Refer to graph in new concepts.

17. 13-17 CHEM 102, Spring 2014, LA TECH 4) Why is instantaneous rates of N 2 O 5 and NO 2 are negative and positive respectively?

18. 13-18 CHEM 102, Spring 2014, LA TECH 2 N 2 O 5 (g) -----> 4 NO 2 (g) + O 2 ( g) Graphing Kinetics Data Average rate =

19. 13-19 CHEM 102, Spring 2014, LA TECH Graph

20. 13-20 CHEM 102, Spring 2014, LA TECH Graph in Problem 7 Time / min [N 2 O 5 ] / moldm - 3 00.01756 200.00933 400.00531 600.00295 800.00167 1000.00094 1600.00014 5) At what time the reaction is complete?

21. 13-21 CHEM 102, Spring 2014, LA TECH Graph in Problem 7 6) Plot this data using excel and attach the graph and do the calculations using the spread sheet: What are the rates of reaction between following min intervals? 0-20 = - ½ [N 2 O 5 ] f - [N 2 O 5 ] i = 2.06 x 10 -4 mol dm -3 min -1 t f - t i 0-20 = - ½ [0.00933] - [0.01756] = 2.06 x 10 -4 mol dm -3 min -1 20 - 0 20-40 = 40-60 = 60-80 =

22. 13-22 CHEM 102, Spring 2014, LA TECH 7) How does reaction rate vary with time in the graph? Consider the decomposition of N 2 O 5.

23. 13-23 CHEM 102, Spring 2014, LA TECH a) Temperature b) Concentration c) Catalysts d) Particle size of solid reactants Factors that affect rates of a chemical reactions

24. 13-24 CHEM 102, Spring 2014, LA TECH 8)What are the main factors that affect a rate of a chemical reaction?

25. 13-25 CHEM 102, Spring 2014, LA TECH Effect of Particle Size on Rate

26. 13-26 CHEM 102, Spring 2014, LA TECH 9) In the graph below, what are the main features regarding rates based on reactants and products and their stoichiometric coefficients and what does it mean by kinetic and equilibrium regions?