1. Thermal Physics Topic 3.2 Thermal Properties of Matter

2. Heat Capacity/Thermal Capacity w When substances undergo the same temperature change they can store or release different amounts of energy w They have different Heat Capacities w Heat capacity =  Q /  T in JK -1  Q = the change in thermal energy in joules  T = the change in temperature in Kelvin w Defined as the amount of energy to change the temperature of a body by unit temperature w Applies to a specific BODY

3. Heat Capacity - 2 w A body with a high heat capacity will take in thermal energy at a slower rate than a substance with a low heat capacity because it needs more time to absorb a greater quantity of thermal energy w They also cool more slowly because they give out thermal energy at a slower rate

4. Specific Heat Capacity w Defined as the amount of thermal energy required to produce unit temperature rise in unit mass of the MATERIAL w Unit mass is normally 1kg, and unit temperature rise is normally 1K w Specific Heat Capacity =  Q / (m  T) w in J kg -1 K -1 where m is the mass of the material

5. w For an object made of 1specific material then w Heat Capacity = m x Specific Heat Capacity

6. Specific Heat Capacity - 2 w Unit masses of different substances contain different numbers of molecules of different types of different masses w If the same amount of internal energy is added to each unit mass it is distributed amongst the molecules

7. Specific Heat capacity - 3 w The average energy change of each molecule will be different for each substance w Therefore the temperature changes will be different w So the specific heat capacities will be different

8. Methods of finding the S.H.C w Two methods Direct Indirect

9. Direct Method - Liquids w Using a calorimeter of known Heat Capacity w (or Specific Heat Capacity of the material and the mass of the calorimeter) w Because Heat Capacity = Mass x Specific Heat Capacity

10. SHC of Liquids Thermometer Calorimeter Heating coil Liquid Insulation StirrerTo joulemeter or voltmeter and ammeter

11. Calculations - Liquids w Electrical Energy input is equal to the thermal energy gained by the liquid and the calorimeter – this is the assumption that we are making w Electrical energy = V x I x t w Energy gained by liquid = m l c l  T l w Energy gained by calorimeter = m c c c  T c

12. Calculations - Liquids -2 w Using conservation of energy w Electrical energy in = thermal energy gained by liquid + thermal energy gained by calorimeter w V x I x t = m l c l  T l + m c c c  T c w The only unknown is the specific heat capacity of the liquid

13. Direct Method - Solids w Using a specially prepared block of the material w The block is cylindrical and has 2 holes drilled in it one for the thermometer and one for the heater Heater hole in the centre, so the heat spreads evenly through the block Thermometer hole, ½ way between the heater and the outside of the block, so that it gets the averge temperature of the block

14. SHC of Solids Insulation Thermometer Heating coil Solid Insulation To joulemeter or voltmeter and ammeter

15. Calculations - Solids w Again using the conservation of energy w Electrical Energy input is equal to the thermal energy gained by the solid w Electrical energy = V x I x t w Energy gained by solid = m s c s  T s

16. Calculations - Solids - 2 w V x I x t = m s c s  T s w The only unknown is the specific heat capacity of the solid

17. Indirect Method w Sometimes called the method of mixtures w In the case of solid, a known mass of solid is heated to a known temperature (usually by immersing in boiling water for a period of time) w Then it is transferred to a known mass of liquid in a calorimeter of known mass

18. Indirect Method cont….. w The change in temperature is recorded and from this the specific heat capacity of the solid can be found w Energy lost by block = Energy gained by liquid and calorimeter w m b c b  T b = m w c w  T w + m c c c  T c the SHC of water and the calorimeter are needed

19. Apparatus Heat Thermometer Beaker Boiling Water Block Thermometer Calorimeter Water Block Insulation

20. Indirect Method – cont…. w In the case of a liquid w A hot solid of known specific heat capacity is transferred to a liquid of unknown specific heat capacity w A similar calculation then occurs

21. Phases (States) of Matter w Matter is defined as anything that has mass and occupies space w There are 4 states of matter w Solids, Liquids, Gases and Plasmas w Most of the matter on the Earth in the form of the first 3 w Most of the matter in the Universe is in the plasma state

22. Macroscopic w Macroscopic properties are all the observable behaviours of that material such as shape, volume, compressibility w The many macroscopic or physical properties of a substance can provide evidence for the nature of that substance

23. Macroscopic Characteristics

24. w These will help to explain what is happening at the atomic level, and this part of the model will be interpreted later

25. Microscopic Characteristics

26. Fluids w Liquids w Gases w are both fluids w Because they FLOW

27. Arrangement of Particles - 1 w Solids Closely packed Strongly bonded to neighbours held rigidly in a fixed position the force of attraction between particles gives them PE

28. Arrangement of Particles - 2 w Liquids Still closely packed Bonding is still quite strong Not held rigidly in a fixed position and bonds can break and reform PE of the particles is higher than a solid because the distance between the particles is higher

29. Arrangement of Particles - 3 w Gases Widely spaced Only interact significantly on closest approach or collision Have a much higher PE than liquids because the particles are furthest apart

30. Changes of State w A substance can undergo changes of state or phase changes at different temperatures w Pure substances have definite melting and boiling points which are characteristic of the substance

31. Changes of State - 2 w The moving particle theory can be used to explain the microscopic behaviour of these phase changes When the solid is heated the particles of the solid vibrate at an increasing rate as the temperature is increased The vibrational KE of the particles increases

32. Changes of State -3 At the melting point a temperature is reached at which the particles vibrate with sufficient thermal energy to break from their fixed positions and begin to slip over each other As the solid continues to melt more and more particles gain sufficient energy to overcome the forces between the particles and over time all the solid particles are changed to a liquid The PE of the system increases as the particles move apart

33. Changes in State - 4 As the heating continues the temperature of the liquid rises due to an increase in the vibrational, rotational and translational energy of the particles At the boiling point a temperature is reached at which the particles gain sufficient energy to overcome the inter-particle forces and escape into the gaseous state. PE increases. Continued heating at the boiling point provides the energy for all the particles to change

34. Heating Curve Solid Liquid Gas Solid - liquid phase change Liquid - gas phase change Temp / o C Time /min

35. Changes of State GASSOLIDLIQUID Freezing/solidification vaporisation condensation melting sublimation Thermal energy given out Thermal energy added

36. Evaporation w The process of evaporation is a change from the liquid state to the gaseous state which occurs at a temperature below the boiling point w The Moving Particle (Kinetic) theory can be applied to understand the evaporation process

37. Explanation w A substance at a particular temperature has a range of particle energies w So in a liquid at any instant, a small fraction of the particles will have KE considerably greater than the average value

38. So w If these particles are near the surface of the liquid, they will have enough KE to overcome the attractive forces of the neighbouring particles and escape from the liquid as a gas w This energy is needed as gases have more PE than liquids.

39. Cooling w Now that the more energetic particles have escaped w The average KE of the remaining particles in the liquid will be lowered w Since temperature is related to the average KE of the particles w A lower KE infers a lower temperature

40. Cool w This is why the temperature of the liquid falls as an evaporative cooling takes place w A substance that cools rapidly is said to be a volatile liquid w When overheating occurs in a human on hot days, the body starts to perspire w Evaporation of the perspiration cools the body

41. Factors Affecting The Rate w Evaporation can be increased by Increasing temperature (more particles have a higher KE) Increasing surface area (more particles closer to the surface) Increasing air flow above the surface (gives the particles somewhere to go to)

42. Latent Heat w The thermal energy which a particle absorbs in melting, vaporising or sublimation or gives out in freezing, condensing or sublimating is called Latent Heat because it does not produce a change in temperature

43. Latent Heat cont…. w When thermal energy is absorbed/released by a body, the temperature may rise/fall, or it may remain constant If the temperature remains constant then a phase change will occur as the thermal energy must either increase the PE of the particles as they move further apart or decrease the PE of the particles as they move closer together

44. Definition w The quantity of heat energy required to change one kilogram of a substance from one phase to another, without a change in temperature is called the Specific Latent Heat of Transformation w Latent Heat =  Q / m in J kg -1

45. Types of Latent Heat w Fusion w Vaporisation w Sublimation w The latent heat of fusion of a substance is less than the latent heat of vaporisation or the latent heat of sublimation

46. Questions w When dealing with questions think about where the heat is being given out where the heat is being absorbed try not to miss out any part

47. Methods of finding Latent Heat w Using similar methods as for specific heat capacity w The latent heat of fusion of ice can be found by adding ice to water in a calorimeter

48. Apparatus Block of ice Thermometer Calorimeter Water Block of ice Insulation

49. w The change in temperature is recorded and from this the latent heat of fusion of the ice can be found w Energy gained by block melting = Energy lost by liquid and calorimeter w m b L b = m w c w  T w + m c c c  T c w the SHC of water and the calorimeter are needed

50. w The latent heat of vaporisation of a liquid could be found by an electrical method

51. Latent Heat of Vaporisation Insulation Thermometer Heating coil Liquid in Calorimeter To joulemeter or voltmeter and ammeter

52. w The initial mass of the liquid is recorded w The change in temperature is recorded for heating the liquid to boiling w The liquid is kept boiling w The new mass is recorded w Energy supplied by heater = energy to raise temperature of liquid + energy use to vaporise some of the liquid w (The calorimeter also needs to be taken in to account. w V I t = m l c l  T l + m e L e + m c c c  T c

53. Pressure w Pressure can be explained by the collisions with the sides of the container w If the temperature increases, the average KE of the particles increases w The increase in velocity of the particles leads to a greater rate of collisions and hence the pressure of the gas increases as the collisions with the side have increased w Also the change in momentum is greater, therefore greater force

54. Pressure continued w When a force is applied to a piston in a cylinder containing a volume of gas w The particles take up a smaller volume w Smaller area to collide with w And hence collisions are more frequent with the sides leading to an increase in pressure

55. w Also, as the piston is being moved in w It gives the particles colliding with it more velocity w Therefore they have more KE w Therefore the temperature of the gas rises.

56. Collisions w Because the collisions are perfectly elastic w There is no loss of KE as a result of the collisions

57. An Ideal Gas w Is a theoretical gas that obeys the gas laws w And thus fit the ideal gas equation exactly

58. Real Gases w Real gases conform to the gas laws under certain limited conditions w But they condense to liquids and then solidify if the temperature is lowered w Furthermore, there are relatively small forces of attraction between particles of a real gas w This is not the case for an ideal gas

59. The Kinetic Theory of Gases w When the moving particle theory is applied to gases it is generally called the kinetic theory w The kinetic theory relates the macroscopic behaviour of an ideal gas to the microscopic behaviour of its molecules or atoms

60. Macroscopic Behaviour w The large number of particles ensures that the number of particles moving in all directions is constant at any time

61. Boyle’s Law w States that the pressure of a fixed mass of gas is inversely proportional to its volume at constant temperature w P  1/V or PV = constant w When the conditions are changed w P 1 V 1 = P 2 V 2

62. The Experiment Air from foot pump Bourdon Pressure gauge Volume of dry air oil

63. What to do w A column of trapped dry air in a sealed tube by the oil w The pressure on this volume of air can be varied by pumping air in or out of the oil reservoir to obtain different pressures w Wait to allow the temperature to return to room temperature

64. The Results P V P 1/ V PV P

65. Charles’ Law w States that the volume of a fixed mass of gas is directly proportional to its absolute temperature at constant pressure w V  T or V/T = constant w When the conditions are changed w V 1 /T 1 = V 2 /T 2

66. The Experiment Tap 1 Tap 2 Tap 3 Water reservoir Fixed mass of gas Mercury in U tube

67. What to do w Fill the mercury column with mercury using the right hand tube (tap 1 open, tap 2 closed) w With tap 1 open drain some mercury using tap 2, then close tap 1 and 2. To trap a fixed mass of gas w Fill the jacket with water (make sure tap 3 is closed)

68. and then w Change the temperature of the water by draining some water from tap 3 and adding hot water w Equalise the pressure by leveling the columns using tap 2 w Read the volume from the scale

69. The Results V T K V T o C A value for absolute zero

70. The Pressure Law w States that the pressure of a fixed mass of gas is directly proportional to its absolute temperature at constant volume w P  T or P/T = constant w When the conditions are changed w P 1 /T 1 = P 2 /T 2

71. The Experiment Bourdon gauge Ice Water Fixed Mass of gas Heat

72. What to do w Change the temperature of the water by heating it w Record the pressure of the gas

73. The Results P T K P T o C A value for absolute zero

74. Absolute Zero and the Kelvin Scale w Charles’ Law and the Pressure Law suggest that there is a lowest possible temperature that substances can go w This is called Absolute Zero w The Kelvin scale starts at this point and increases at the same scale as the Celsius Scale

75. w Therefore -273 o C is equivalent to 0 K w ∆1 o C is the same as ∆1 K w To change o C to K, add 273 w To change K to o C, subtract 273

76. Combining the Laws w The gas laws can be combined to give a single equation w For a fixed mass of gas its pressure times its volume divided by its absolute temperature is a constant w PV/T = k w So that P 1 V 1 /T 1 = P 2 V 2 /T 2

77. The Ideal Gas Equation w PV = nRT w Where n is the number of moles w R is the universal gas constant 8.31 J mol -1 K -1

78. An Ideal Gas w Is a theoretical gas that obeys the gas laws w And thus fit the ideal gas equation exactly

79. Real Gases w Real gases conform to the gas laws under certain limited conditions w But they condense to liquids and then solidify if the temperature is lowered w Furthermore, there are relatively small forces of attraction between particles of a real gas w This is not the case for an ideal gas

80. The Kinetic Theory of Gases w When the moving particle theory is applied to gases it is generally called the kinetic theory w The kinetic theory relates the macroscopic behaviour of an ideal gas to the microscopic behaviour of its molecules or atoms

81. The Postulates w Gases consist of tiny particles called atoms or molecules w The total number of particles in a sample is very large w The particles are in constant random motion w The range of the intermolecular forces is small compared to the average separation

82. The Postulates continued w The size of the particles is relatively small compared with the distance between them w Collisions of a short duration occur between particles and the walls of the container w Collisions are perfectly elastic

83. The Postulates continued w No forces act between the particles except when they collide w Between collisions the particles move in straight lines w And obey Newton’s Laws of motion

84. Macroscopic Behaviour w The large number of particles ensures that the number of particles moving in all directions is constant at any time

85. Pressure w Pressure can be explained by the collisions with the sides of the container w If the temperature increases, the average KE of the particles increases w The increase in velocity of the particles leads to a greater rate of collisions and hence the pressure of the gas increases as the collisions with the side have increased w Also the change in momentum is greater, therefore greater force

86. Pressure continued w When a force is applied to a piston in a cylinder containing a volume of gas w The particles take up a smaller volume w Smaller area to collide with w And hence collisions are more frequent with the sides leading to an increase in pressure

87. w Also, as the piston is being moved in w It gives the particles colliding with it more velocity w Therefore they have more KE w Therefore the temperature of the gas rises.

88. Collisions w Because the collisions are perfectly elastic w There is no loss of KE as a result of the collisions