1. Reaction Energy and Reaction Kinetics Chapter 17 Notes

2. Thermochemistry Thermochemistry is the study of the transfers of energy as heat that accompany chemical reactions and physical changes. –Endothermic and exothermic reactions –Phase changes and specific heat

3. Calorimeter The energy absorbed or released as heat in a chemical or physical change is measured in a calorimeter.

4. Heat and Temperature Heat (q): energy transferred between samples of matter because of a difference in their temperatures. Temperature: a measure of the average kinetic energy of the particles in a sample of matter. –Higher temperature = faster particles –Lower temperature = slower particles

5. Heat As an object absorbs heat –the particles increase in kinetic energy –the temperature of the object increases Heat always flows from a __________object to a __________ object hotter colder

6. Thermochemical Systems System: the collection of matter that you are studying –The liquid in which a reaction is taking place –The interior of a calorimeter Surroundings: the area directly around the system that is capable of absorbing energy from or releasing energy to your system –The beaker holding the liquid and the air around the beaker –The walls of the calorimeter and the air around them

7. Law of Conservation of Energy Energy cannot be created or destroyed. It can be moved from place to place

8. Endothermic Process An endothermic process absorbs heat from its surroundings –Instant cold packs –Vinegar and baking soda –Boiling water

9. Exothermic Process A system that releases energy to its surroundings –Diluting sulfuric acid –Water freezing into ice –The heating unit included in MREs

10. Heat of Reaction The energy transferred as heat during a chemical reaction is called the heat of reaction. This heat is shown as either a reactant or a product in a thermochemical equation. –CH 4 + 2 O 2 → CO 2 + 2 H 2 O + 1565 J –CH 3 COOH + NaHCO 3 + 1245 J → NaC 2 H 3 O 2 + CO 2 + H 2 O Exothermic Endothermic

11. Enthalpy Enthalpy change: the amount of energy transferred as heat during a process occurring at constant pressure ΔH = H products – H reactants –Positive for endothermic reactions –Negative for exothermic reactions

12. Enthalpy and Thermochemical Equations Exothermic reaction CH 4 + 2 O 2 → CO 2 + 2 H 2 O + 1565 J ΔH =-1565 J Endothermic reaction CH 3 COOH + NaHCO 3 + 1245 J → NaC 2 H 3 O 2 + CO 2 + H 2 O ΔH =1245 J

13. Entropy Entropy: the amount of disorder within a system –High entropy = chaotic The plasma inside the sun Typical kid’s bedroom –Low entropy = very orderly Ice My movie collection Processes occur spontaneously (without an external driving force) if they increase the entropy of the system.

14. Units for Heat calorie (cal) = the amount of heat needed to raise the temperature of 1 gram of water by 1 o C. The “c” is ALWAYS lowercase for this unit. Calorie (Cal) = 1 kilocalorie (kcal). This is what we mean when we talk about food – how much energy is in the food. The “C” is ALWAYS capitalized! Joule = SI unit for energy, including heat

15. Heat Capacity The amount of heat needed to change an object’s temperature. This depends on –Size of the object –Material of the object –How big is the temperature change To allow more direct comparisons we use specific heat capacity instead.

16. Specific Heat Capacity The amount of heat need to change the temperature of 1 gram of a material by 1 o C –For water, c = 4.18 J/g∙ o C –This means it takes 4.18 joules of energy to raise the temperature of 1 gram of water from 20 o C to 21 o C You have been given a table of specific heats. This needs to go in the references section of your binder.

17. Calculating Specific Heat Heat (J or cal) Change in temperature = T final – T initial ( o C or K) Mass (g) Specific heat (J/g∙ o C or cal/g∙ o C)

18. Example 1 The temperature of a piece of copper with a mass of 95.4 grams increases from 25.0 o C to 48.0 o C when the metal absorbs 849 J of heat. What is the specific heat of copper?

19. Example 2 How much heat is required to raise the temperature of 250.0 g of mercury 52.0 o C?

20. Example 3 What is the temperature change when 2543 J of heat are added to 76.4 g of alcohol?

21. Example 4 The temperature of a 283 gram sample increases 11.2 o C by absorbing 1204 J of heat. What material is the sample?

22. Reaction Kinetics Chemical kinetics: the study of reaction rates and mechanisms –How quickly reactions take place –The actual process of the reaction

23. Reaction Mechanisms Mechanism: the step-by-step sequence of reactions by which the overall chemical change occur. Rate determining step: the slowest part of the reaction mechanism –It takes the longest, thus determining the speed of the overall reaction –When baking slice and bake cookies, the actual baking is the longest step. It determines how long it takes to bake those cookies.

24. Reaction Mechanisms: An Example The reaction 2 A 2 B + CD 4 → CB 2 + 4 AD doesn’t happen all at once. Instead it follows the following reaction mechanism. 1 st : 2 A 2 B → 4 A - + 2 B 2+ (very fast) 2 nd : 4 A - +CD 4 → C 4+ + 4 AD (very slow) 3 rd : C 4+ + 2 B 2+ → CB 2 (very fast)

25. What is Needed for a Reaction? The reactants in question must collide with: –Enough energy –Favorable orientation Anything that increases the likelihood of those two conditions being met will increase the reaction rate

26. Kinetics and Conditions 1.Nature of reactants – some elements react more quickly than other elements 2.Surface area – more surface area means more opportunities for favorable collisions 3.Temperature – hotter reactants will collide with more energy 4.Concentration – more concentrated solutions allow for more frequent collisions

27. Chemical Reaction Rates Reaction rate: how quickly the concentration of a substance in a chemical reaction is changing. It’s measured in M/s. Instantaneous reaction rate: the rate at any given instant of time Initial reaction rate: the rate when a reaction is first started

28. Reaction Rates For reactants, the reaction rate is how quickly the concentration is decreasing For products, the reaction rate is how quickly the concentration is increasing

29. Rate Expressions Rate law/rate expression: an equation that relates reaction rate and concentrations of reactants **Important note** You cannot predict the values of n, m, or p from the reaction equation. The rate law must be determined experimentally!

30. Rate Expressions Rate constant, k: –A proportionality constant that allows the direct calculation of the rate from the concentrations of the reactants and catalyst –The units of k vary according to the rate law: you use the units needed to make the units for the rate what you need. They will usually be one of the following:

31. The Order of Reaction Total reaction order: the sum of all of the exponents in the rate law Common orders – –0 th : rate = k –1 st : rate = k[A] –2 nd : rate = k[A][B] or rate = k[A] 2 –3 rd : rate = k[A][B][C], rate = k[A] 2 [B] or rate = k[A] 3 NOTE: higher reaction orders have more possibilities for the rate law

32. Determination of the Rate Expression We need to determine how each change in concentration affected the reaction rate. Run[A] (M)[B] (M)[C] (M)Rate (M/s) 10.10 0.00080 20.200.10 0.0016 30.100.200.100.00080 40.10 0.200.0032

33. Determination of the Rate Expression First, what changes between run 1 and run 2? –The concentration of A is doubled Run[A] (M)[B] (M)[C] (M)Rate (M/s) 10.10 0.00080 20.200.10 0.0016 30.100.200.100.00080 40.10 0.200.0032

34. Determination of the Rate Expression What change does this bring in the rate? –The rate is also doubled –So a change in [A] causes the same change in rate –Rate [A] Run[A] (M)[B] (M)[C] (M)Rate (M/s) 10.10 0.00080 20.200.10 0.0016 30.100.200.100.00080 40.10 0.200.0032

35. Determination of the Rate Expression Next, what changes between run 1 and run 3? –The concentration of B is doubled Run[A] (M)[B] (M)[C] (M)Rate (M/s) 10.10 0.00080 20.200.10 0.0016 30.100.200.100.00080 40.10 0.200.0032

36. Determination of the Rate Expression What change does this bring in the rate? –The rate is not changed –So a change in [B] does not change the rate Run[A] (M)[B] (M)[C] (M)Rate (M/s) 10.10 0.00080 20.200.10 0.0016 30.100.200.100.00080 40.10 0.200.0032

37. Determination of the Rate Expression Next, what changes between run 1 and run 3? –The concentration of C is doubled Run[A] (M)[B] (M)[C] (M)Rate (M/s) 10.10 0.00080 20.200.10 0.0016 30.100.200.100.00080 40.10 0.200.0032

38. Determination of the Rate Expression What change does this bring in the rate? –The rate is quadrupled –So a change in [C] is squared in the rate –Rate [C] 2 Run[A] (M)[B] (M)[C] (M)Rate (M/s) 10.10 0.00080 20.200.10 0.0016 30.100.200.100.00080 40.10 0.200.0032

39. Determination of the Rate Expression When we put it all together we get –Rate = k[A][C] 2 Run[A] (M)[B] (M)[C] (M)Rate (M/s) 10.10 0.00080 20.200.10 0.0016 30.100.200.100.00080 40.10 0.200.0032

40. Reaction Energy Diagrams Shows the changes in energy as a reaction takes place Can be used to analyze many energy changes that occur during a reaction

41. Reaction Energy Diagrams A: energy held by the activated complex B: energy of the reactants C: energy of the products F: heat of reaction I: activation energy

42. Reaction Energy Diagrams This is an exothermic reaction – the reactants have more energy than the products, so energy has been released

43. Reaction Energy Diagrams This is an endothermic reaction – the reactants have less energy than the products, so energy has been absorbed

44. Energy During Reaction Transition state energy: the energy held by the activated complex during a reaction Activated complex: a molecule that temporarily exists during the process of a reactions (i.e., it is created in the reaction mechanism) Activation energy: the energy required to start a reaction (the spark from a match when lighting a gas burner, for example)

45. Changing the Energy Requirements Catalyst: a substance that speeds a reaction up by decreasing the activation energy required –Homogeneous catalyst: in the same state as the reactants –Heterogeneous catalyst: in a different state than the reactants Inhibitor: a substance that slows a reaction down by increasing the activation energy required

46. Reaction Energy Diagrams D: catalyzed reaction E: inhibited reaction