1. Chapter 10 Energy

2. Chapter 10 Table of Contents Copyright © Cengage Learning. All rights reserved 2 10.1 The Nature of Energy 10.2 Temperature and Heat 10.3 Exothermic and Endothermic Processes 10.4 Thermodynamics 10.5 Measuring Energy Changes 10.6Thermochemistry (Enthalpy) 10.7 Hess’s Law 10.8 Quality Versus Quantity of Energy 10.9 Energy and Our World 10.10Energy as a Driving Force

3. Section 10.1 The Nature of Energy Return to TOC Copyright © Cengage Learning. All rights reserved 3 Ability to do work or produce heat. That which is needed to oppose natural attractions. Law of conservation of energy – energy can be converted from one form to another but can be neither created nor destroyed.  The total energy content of the universe is constant. Energy

4. Section 10.1 The Nature of Energy Return to TOC Copyright © Cengage Learning. All rights reserved 4 Potential energy – energy due to position or composition. Kinetic energy – energy due to motion of the object and depends on the mass of the object and its velocity. Energy is the capacity to do work. Radiant energy - comes from the sun and is earth’s primary energy source Thermal energy - is the energy associated with the random motion of atoms and molecules Chemical energy - is the energy stored within the bonds of chemical substances Nuclear energy is the energy stored within the collection of neutrons and protons in the atom Energy

5. Section 10.1 The Nature of Energy Return to TOC Copyright © Cengage Learning. All rights reserved 5 In the initial position, ball A has a higher potential energy than ball B. Initial Position

6. Section 10.1 The Nature of Energy Return to TOC Copyright © Cengage Learning. All rights reserved 6 After A has rolled down the hill, the potential energy lost by A has been converted to random motions of the components of the hill (frictional heating) and to the increase in the potential energy of B. Final Position

7. Section 10.1 The Nature of Energy Return to TOC Copyright © Cengage Learning. All rights reserved 7 Heat involves the transfer of energy between two objects due to a temperature difference. Work – force acting over a distance. Energy is a state function; work and heat are not:  State Function – property that does not depend in any way on the system’s past or future (only depends on present state).  Changes independently of its pathway Energy

8. Section 10.1 The Nature of Energy Return to TOC Copyright © Cengage Learning. All rights reserved 8 State functions are properties that are determined by the state of the system, regardless of how that condition was achieved. Potential energy of hiker 1 and hiker 2 is the same even though they took different paths. energy, pressure, volume, temperature  U = U final - U initial  P = P final - P initial  V = V final - V initial  T = T final - T initial

9. Section 10.2 Temperature and Heat Return to TOC Copyright © Cengage Learning. All rights reserved 9 A measure of the random motions of the components of a substance. Temperature Temperature is a measure of the thermal energy.

10. Section 10.2 Temperature and Heat Return to TOC Copyright © Cengage Learning. All rights reserved 10 A flow of energy between two objects due to a temperature difference between the objects.  Heat is the way in which thermal energy is transferred from a hot object to a colder object. Heat

11. Section 10.3 Exothermic and Endothermic Processes Return to TOC Copyright © Cengage Learning. All rights reserved 11 System – part of the universe on which we wish to focus attention. Surroundings – include everything else in the universe.

12. Section 10.3 Exothermic and Endothermic Processes Return to TOC Copyright © Cengage Learning. All rights reserved 12 open mass & energy Exchange: closed Energy exchange isolated No exchange

13. Section 10.3 Exothermic and Endothermic Processes Return to TOC Copyright © Cengage Learning. All rights reserved 13 Energy Changes Accompanying the Burning of a Match

14. Section 10.3 Exothermic and Endothermic Processes Return to TOC Copyright © Cengage Learning. All rights reserved 14 Endothermic Process:  Heat flow is into a system.  Absorb energy from the surroundings. Exothermic Process:  Energy flows out of the system. Energy gained by the surroundings must be equal to the energy lost by the system.

15. Section 10.3 Exothermic and Endothermic Processes Return to TOC Copyright © Cengage Learning. All rights reserved 15 Concept Check Is the freezing of water an endothermic or exothermic process? Explain.

16. Section 10.3 Exothermic and Endothermic Processes Return to TOC Copyright © Cengage Learning. All rights reserved 16 Concept Check Classify each process as exothermic or endothermic. Explain. The system is underlined in each example. a)Your hand gets cold when you touch ice. b)The ice gets warmer when you touch it. c)Water boils in a kettle being heated on a stove. d)Water vapor condenses on a cold pipe. e)Ice cream melts. Exo Endo Exo Endo

17. Section 10.3 Exothermic and Endothermic Processes Return to TOC Copyright © Cengage Learning. All rights reserved 17 Concept Check For each of the following, define a system and its surroundings and give the direction of energy transfer. a)Methane is burning in a Bunsen burner in a laboratory. b)Water drops, sitting on your skin after swimming, evaporate.

18. Section 10.3 Exothermic and Endothermic Processes Return to TOC Copyright © Cengage Learning. All rights reserved 18 Concept Check Hydrogen gas and oxygen gas react violently to form water.  Which is lower in energy: a mixture of hydrogen and oxygen gases, or water? Explain.

19. Section 10.3 Exothermic and Endothermic Processes Return to TOC Copyright © Cengage Learning. All rights reserved 19 H 2 + O 2 have higher potential energy than H 2 O energy is given offenergy is absorbed Electrolysis of Water Burning of Hydrogen in Air higher potential energylower potential energy

20. Section 10.4 Thermodynamics Return to TOC Copyright © Cengage Learning. All rights reserved 20 Study of energy Law of conservation of energy is often called the first law of thermodynamics.  The energy of the universe is constant.

21. Section 10.5 Measuring Energy Changes Return to TOC Copyright © Cengage Learning. All rights reserved 21 The common energy units for heat are the calorie and the joule.  calorie – the amount of energy (heat) required to raise the temperature of one gram of water 1 o C.  Joule – 1 calorie = 4.184 joules  1Cal (food) = 1000 calories

22. Section 10.5 Measuring Energy Changes Return to TOC Copyright © Cengage Learning. All rights reserved 22 Convert 60.1 cal to joules. Example

23. Section 10.5 Measuring Energy Changes Return to TOC Copyright © Cengage Learning. All rights reserved 23 1.The amount of substance being heated (number of grams). 2.The temperature change (number of degrees). 3.The identity of the substance.  Specific heat capacity is the energy required to change the temperature of a mass of one gram of a substance by one Celsius degree. Energy (Heat) Required to Change the Temperature of a Substance Depends On:

24. Section 10.5 Measuring Energy Changes Return to TOC Copyright © Cengage Learning. All rights reserved 24 Specific Heat Capacities of Some Common Substances

25. Section 10.5 Measuring Energy Changes Return to TOC Copyright © Cengage Learning. All rights reserved 25 Energy (heat) required, Q = s × m × ΔT Q = energy (heat) required (J) s = specific heat capacity (J/°C·g) m = mass (g) ΔT = change in temperature (°C) To Calculate the Energy Required for a Reaction:

26. Section 10.5 Measuring Energy Changes Return to TOC Copyright © Cengage Learning. All rights reserved 26 Calculate the amount of heat energy (in joules) needed to raise the temperature of 6.25 g of water from 21.0°C to 39.0°C. Where are we going? We want to determine the amount of energy needed to increase the temperature of 6.25 g of water from 21.0°C to 39.0°C. What do we know? The mass of water and the temperature increase. Example

27. Section 10.5 Measuring Energy Changes Return to TOC Copyright © Cengage Learning. All rights reserved 27 Calculate the amount of heat energy (in joules) needed to raise the temperature of 6.25 g of water from 21.0°C to 39.0°C. What information do we need? We need the specific heat capacity of water.  4.184 J/g°C How do we get there? Example

28. Section 10.5 Measuring Energy Changes Return to TOC Copyright © Cengage Learning. All rights reserved 28 Exercise A sample of pure iron requires 142 cal of energy to raise its temperature from 23ºC to 92ºC. What is the mass of the sample? (The specific heat capacity of iron is 0.45 J/gºC.) a)0.052 g b)4.6 g c)19 g d)590 g

29. Section 10.5 Measuring Energy Changes Return to TOC Copyright © Cengage Learning. All rights reserved 29 Twice as much heat energy is required to raise the temperature of 200 g of water 10 o C as compared to 100 g of water. 200 g water 20 o C A 100 g water 20 o C B 100 g water 30 o C 200 g water 30 o C heat beakers 4184 J 8368 J temperature rises 10 o C

30. Section 10.5 Measuring Energy Changes Return to TOC Copyright © Cengage Learning. All rights reserved 30 Concept Check A 100.0 g sample of water at 90°C is added to a 100.0 g sample of water at 10°C. The final temperature of the water is: a) Between 50°C and 90°C b) 50°C c) Between 10°C and 50°C

31. Section 10.5 Measuring Energy Changes Return to TOC Copyright © Cengage Learning. All rights reserved 31 Concept Check A 100.0 g sample of water at 90.°C is added to a 500.0 g sample of water at 10.°C. The final temperature of the water is: a) Between 50°C and 90°C b) 50°C c) Between 10°C and 50°C Calculate the final temperature of the water. 23°C

32. Section 10.5 Measuring Energy Changes Return to TOC Copyright © Cengage Learning. All rights reserved 32 Concept Check You have a Styrofoam cup with 50.0 g of water at 10.  C. You add a 50.0 g iron ball at 90.  C to the water. (s H2O = 4.18 J/°C·g and s Fe = 0.45 J/°C·g) The final temperature of the water is: a) Between 50°C and 90°C b) 50°C c) Between 10°C and 50°C Calculate the final temperature of the water. 18°C

33. Section 10.6 Thermochemistry (Enthalpy) Return to TOC Copyright © Cengage Learning. All rights reserved 33 Calorimetry Enthalpy, H is measured using a calorimeter.

34. Section 10.6 Thermochemistry (Enthalpy) Return to TOC Copyright © Cengage Learning. All rights reserved 34 An energy transformation occurs whenever a chemical change occurs. If energy is absorbed during a chemical change, the products will have more chemical potential energy than the reactants. If energy is given off in a chemical change, the products will have less chemical potential energy than the reactants.

35. Section 10.6 Thermochemistry (Enthalpy) Return to TOC Copyright © Cengage Learning. All rights reserved 35 A sample of a metal with a mass of 212 g is heated to 125.0 o C and then dropped into 375 g of water at 240.0 o C. If the final temperature of the water is 34.2 o C, what is the specific heat of the metal? When the metal enters the water, it begins to cool, losing heat to the water. At the same time, the temperature of the water rises. This process continues until the temperature of the metal and the temperature of the water are equal, at which point (34.2 o C) no net flow of heat occurs.

36. Section 10.6 Thermochemistry (Enthalpy) Return to TOC Copyright © Cengage Learning. All rights reserved 36 A sample of a metal with a mass of 212 g is heated to 125.0oC and then dropped into 375 g of water at 240.0oC. If the final temperature of the water is 34.2oC, what is the specific heat of the metal? Calculate the heat gained by the water. Calculate the final temperature of the metal. Calculate the specific heat of the metal.

37. Section 10.6 Thermochemistry (Enthalpy) Return to TOC Copyright © Cengage Learning. All rights reserved 37 A sample of a metal with a mass of 212 g is heated to 125.0oC and then dropped into 375 g of water at 240.0oC. If the final temperature of the water is 34.2oC, what is the specific heat of the metal? Δt = 34.2 o C – 24.0 o C = 10.2 o C temperature rise of the water Heat Gained by the Water heat gained by the water =

38. Section 10.6 Thermochemistry (Enthalpy) Return to TOC Copyright © Cengage Learning. All rights reserved 38 A sample of a metal with a mass of 212 g is heated to 125.0oC and then dropped into 375 g of water at 240.0oC. If the final temperature of the water is 34.2oC, what is the specific heat of the metal? Δt = 125.0 o C – 34.2 o C = 90.8 o C temperature drop of the metal Once the metal is dropped into the water, its temperature will drop until it reaches the same temperature as the water (34.2 o C). Heat Lost by the Metal heat lost by the metal heat gained by the water = =

39. Section 10.6 Thermochemistry (Enthalpy) Return to TOC Copyright © Cengage Learning. All rights reserved 39 A sample of a metal with a mass of 212 g is heated to 125.0oC and then dropped into 375 g of water at 240.0oC. If the final temperature of the water is 34.2oC, what is the specific heat of the metal? specific heat of the metal = The heat lost or gained by the system is given by: (mass) (specific heat) (Δt) = energy change rearrange

40. Section 10.6 Thermochemistry (Enthalpy) Return to TOC Copyright © Cengage Learning. All rights reserved 40 Homework Reading assignment –Pages 288 through 302 and chapter review Homework Questions and Problems: pages 317 - 319 –3, 5, 9, 13, 17, 19, 25, 27, 29, 31, 33, 35. Due on