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# 17 heat and thermodynamic

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### 17 heat and thermodynamic

1. 1. Heat and Thermodynamic Topic 16
2. 2. Lecture Outline <ul><ul><ul><li>16.1 Heat as Energy Transfer </li></ul></ul></ul><ul><ul><ul><li>16.2 Internal Energy </li></ul></ul></ul><ul><ul><ul><li>16.3 Specific Heat </li></ul></ul></ul><ul><ul><ul><li>16.4 Latent Heat </li></ul></ul></ul><ul><ul><ul><li>16.5 Heat Transfer </li></ul></ul></ul>
3. 3. 16.1 Heat As Energy Transfer We often speak of heat as though it were a material that flows from one object to another; it is not. Rather, it is a form of energy. In the eighteenth century – heat flow considered as movement of fluid substance call caloric In the nineteenth century – heat considered to be akin to work
4. 4. <ul><li>Unit of heat: calorie (cal) </li></ul><ul><li>1 cal is the amount of heat necessary to raise the temperature of 1 g of water by 1 Celsius degree. </li></ul><ul><li>Please note – the calories on our food labels are really kilocalories (kcal or Calories), the heat necessary to raise 1 kg of water by 1 Celsius degree. </li></ul>
5. 5. If heat is a form of energy, it ought to be possible to equate it to other forms. The experiment by James Prescott Joule below found the mechanical equivalent of heat by using the falling weight to heat the water:
6. 6. Definition of heat: Heat is energy transferred from one object to another because of a difference in temperature.
7. 7. <ul><li>Example 19-1 Working the extra Calories </li></ul><ul><li>Suppose you throw caution to the wind and eat too much ice cream and cake on the order of 500 Calories (kcal). To compensate, you want to do an equivalent amount of work climbing stairs or a mountain. How much total height must you climb? For this calculation, take your mass to be about 60 kg. </li></ul>
8. 8. 16.2 Internal Energy The sum total of all the energy of all the molecules in a substance is its internal (or thermal) energy. Temperature: measures molecules’ average kinetic energy Heat: transfer of energy due to difference in temperature Internal energy: total energy of all molecules
9. 9. Internal energy of an ideal gas: can also be written:
10. 10. 16.3 Specific Heat The amount of heat required to change the temperature of a material is proportional to the mass and to the temperature change: The specific heat, c , is characteristic of the material. Some values are listed at right.
11. 11. <ul><li>Example 19-2 Heat transferred depends on specific heat </li></ul><ul><li>a) How much heat input is needed to rise the temperature of an empty 20 kg vat made of iron from 10 °C to 90°C? </li></ul><ul><li>(iron: c = 450 J/kg C°) </li></ul><ul><li>b) What if the vat is filled with 20 kg of water? </li></ul><ul><li>(water: c = 4186 J/kg C°) </li></ul>
12. 12. Calorimetry – Solving Problems Closed system: no mass enters or leaves, but energy may be exchanged with the environment Open system: mass may transfer as well Isolated system: closed system where no energy in any form is transferred For an isolated system, Energy out of one part = energy into another part Or: heat lost = heat gained
13. 13. <ul><li>Example 19-3 The cup cools the tea </li></ul><ul><li>If 200 cm 2 of tea at 95 °C is poured into a 150 g glass cup initially at 25°C, what will be the common final temperature T of the tea and the cup when equilibrium is reaches, assuming no heat flow to the surroundings? </li></ul><ul><li>(water: c = 4186 J/kg C°, ρ = 1000 kg/m 3 ) </li></ul><ul><li>(glass: c = 840 J/kg C°) </li></ul>
14. 14. The instrument to the left is a calorimeter, which makes quantitative measurements of heat exchange. A sample is heated to a well-measured high temperature, plunged into the water, and the equilibrium temperature measured. This gives the specific heat of the sample.
15. 15. <ul><li>Example 19-4 Unknown specific heat determined by calorimetry </li></ul><ul><li>An engineer wishes to determine the specific heat of a new metal alloy. A 0.150 kg sample of the alloy is heated to 540 °C. It is then quickly placed in 400 g of water at 10.0°C, which is contained in a 200 g aluminum calorimeter. The final temperature of the system is 30.5ºC. Calculate the specific heat of the alloy. </li></ul><ul><li>(water: c = 4186 J/kg C°) </li></ul><ul><li>(aluminum: c = 900 J/kg C°) </li></ul>
16. 16. Another type of calorimeter is called a bomb calorimeter; it measures the thermal energy released when a substance burns. This is the way the Caloric content of foods is measured.
17. 17. <ul><li>Example: Measuring the energy content of a cookie </li></ul><ul><li>Determine the energy content of 100 g of Fahlgren’s fudge cookies from the following measurements. A 10 g sample of a cookie is allowed to dry before putting it in a bomb calorimeter. The aluminum bomb has a mass of 0.615 kg and is placed in 2.00 kg of water contained in an aluminum calorimeter cup of mass 0.524 kg. The initial temperature of the system is 15.0 ºC, and its temperature after ignition is 36.0ºC. </li></ul><ul><li>(water: c = 4186 J/kg C°) </li></ul><ul><li>(aluminum: c = 900 J/kg C°) </li></ul>
18. 18. 16.4 Latent Heat Energy is required for a material to change phase, even though its temperature is not changing.
19. 19. Heat of fusion, L F : heat required to change 1.0 kg of material from solid to liquid Heat of vaporization, L V : heat required to change 1.0   kg of material from liquid to vapor
20. 20. The total heat required for a phase change depends on the total mass and the latent heat:
21. 21. <ul><li>Example: Making ice </li></ul><ul><li>How much energy does a freezer have to remove from 1.5 kg of water at 20 °C to make ice at -12°C? </li></ul><ul><li>(water: c = 4186 J/kg C°; L F = 333 kJ/kg) </li></ul><ul><li>(ice: c = 2100 J/kg C°) </li></ul>
22. 22. <ul><li>Example 19-5 Will all the ice melt? </li></ul><ul><li>At a reception, a 0.50 kg chunk of ice at -10 °C is placed in 3.0 kg of “iced” tea at 20°C. At what temperature and in what phase will the final mixture will be? The tea can be considered as water. Ignore any heat flow to the surroundings, including the container. </li></ul><ul><li>(water: c = 4186 J/kg C°; L F = 333 kJ/kg) </li></ul><ul><li>(ice: c = 2100 J/kg C°) </li></ul>
23. 23. <ul><li>Example 19-9 Determining a latent heat </li></ul><ul><li>The specific heat of a liquid mercury is 140 J/kg C °. When 1.0 kg of solid mercury at its melting point of -39°C is placed in a 0.50 kg aluminum calorimeter filled with 1.2 kg of water at 20.0°C, the final temperature of the combination is found to be 16.5°C. What is the heat of fusion of mercury in J/kg </li></ul>
24. 24. The latent heat of vaporization is relevant for evaporation as well as boiling. The heat of vaporization of water rises slightly as the temperature decreases. On a molecular level, the heat added during a change of state does not go to increasing the kinetic energy of individual molecules, but rather to break the close bonds between them so the next phase can occur.
25. 25. 16.5 Heat Transfer Conduction Heat conduction can be visualized as occurring through molecular collisions. The heat flow per unit time is given by:
26. 26. The constant k is called the thermal conductivity. Materials with large k are called conductors; those with small k are called insulators.
27. 27. <ul><li>Example 19-13 Heat loss through windows </li></ul><ul><li>A major source of heat loss from a house is through the windows. Calculate the rate of heat flow through a glass windows 2.0 m × 1.5 m in area and 3.2 mm thick, if the temperatures at the inner and outer surfaces are 15.0°C and 14.0°C, respectively. </li></ul>
28. 28. Building materials are measured using R − values (thermal resistance) rather than thermal conductivity: Here, l is the thickness of the material.
29. 29. Convection Convection occurs when heat flows by the mass movement of molecules from one place to another. It may be natural or forced; both these examples are natural convection.
30. 30. Many home heating systems are forced hot-air systems; these have a fan that blows the air out of registers, rather than relying completely on natural convection. Our body temperature is regulated by the blood; it runs close to the surface of the skin and transfers heat. Once it reaches the surface of the skin, the heat is released through convection, evaporation, and radiation.
31. 31. Radiation The most familiar example of radiation is our own Sun, which radiates at a temperature of almost 6000 K.
32. 32. The energy radiated has been found to be proportional to the fourth power of the temperature: The constant σ is called the Stefan-Boltzmann constant: The emissivity e is a number between zero and one characterizing the surface; black objects have an emissivity near one, while shiny ones have an emissivity near zero.
33. 33. <ul><li>Every object emits and absorb energy by radiation to another object </li></ul><ul><li>The net rate if radiant heat flow from the object is given by the equation: </li></ul>
34. 34. <ul><li>Example 19-14 Cooling by radiation </li></ul><ul><li>An athlete is sitting unclothed in a locker room whose dark walls are at a temperature of 15 °C. Estimate the rate of heat loss by radiation, assuming a skin temperature of 34°C and e =0.70. Take the surface area of the body not in contact with the chair to be 1.5 m 2 . </li></ul>
35. 35. If you are sitting in a place that is too cold, your body radiates more heat than it can produce. You will start shivering and your metabolic rate will increase unless you put on warmer clothing.
36. 36. If you are in the sunlight, the Sun’s radiation will warm you. In general, you will not be perfectly perpendicular to the Sun’s rays, and will absorb energy at the rate:
37. 37. This cos θ effect is also responsible for the seasons.
38. 38. <ul><li>Example: Getting a tan – energy absorption </li></ul><ul><li>What is the rate of energy absorption from the Sun by a person lying flat on the beach on a clear day if the Sun makes a 30 ° angle with the vertical? Assume that e = 0.70, that 1000 W/m 2 reaches the Earth’s surface and a typical human has an area A = 0.8 m 2 . </li></ul>
39. 39. Thermography – the detailed measurement of radiation from the body – can be used in medical imaging. Warmer areas may be a sign of tumors or infection; cooler areas on the skin may be a sign of poor circulation.