1. Topic 3 Thermal physics

2. Learn the definitions. We will be having a definitions test next Thursday 10 th December. Homework

3. What is Temperature?

4. Temperature TEMPERATURE determines the direction of flow of thermal energy between two bodies in thermal contact HOT COLD This is another way of saying that if an object is hotter than another, heat energy will flow from the hotter object to the colder! Obvious, but important to remember!

5. Temperature Temperature is also a measure of the average random kinetic energy of the particles in a substance. Note that they are not all travelling at the same speed.

6. Temperature The hotter the temperature, the faster the average speed of the particles Note that they are not all travelling at the same speed.

7. Thermal equilibrium Two bodies in thermal contact will eventually reach the same temperature. The two bodies are now said to be in thermal equilibrium. WARM

8. Measuring Temperature In 1742, Andreas Celcius created the temperature scale that is known by his name. I’ve never heard of the Andreas scale, it must be a European thing

9. Celcius Scale In the Celcius scale, a value of zero degrees is assigned to the freezing point of water, and a value of one hundred degrees to the boiling point of water.

10. Making a Celcius thermometer Place a glass tube containing mercury in a mixture of ice and water and labelling the position of the mercury as zero. 0°C

11. Making a Celcius thermometer Then place the tube in boiling water and label the new length as 100°C. 0°C 100°C

12. Making a Celcius thermometer Finally the range from 0 to 100 is subdivided into equal intervals. 0°C 100°C

13. Kelvin Temperature Lord Kelvin 1824-1907

14. Pressure and Temperature http://phet.colorado.edu/sims/ideal- gas/gas-properties_en.jnlphttp://phet.colorado.edu/sims/ideal- gas/gas-properties_en.jnlp

15. Kelvin Temperature Kelvin temperature is proportional to the average random kinetic energy of the particles in a substance. Note that they are not all travelling at the same speed.

16. Absolute/Kelvin temperature and Celsius T (in Kelvin) = T (in degrees Celcius) + 273 Just to mention for now that zero Kelvin is the lowest possible temperature.

17. Measuring temperature The thermometer has to be placed in thermal contact with whatever is being measured until the thermometer and object are in thermal equilibrium. 0°C 100°C We’ll measure some temperatures in a moment

18. So what is heat?

19. Heat is the amount of thermal energy. For example, the sparks from a sparkler are at around 800°C but do not burn your skin. However, a hot cup of tea at around 100°C will burn your hand badly. This is because the tea contains more heat energy, even though it is cooler.

20. Internal Energy This is the sum of the kinetic energies and potential energies of the particles in a substance If you imagine the forces between particles as a spring, you can see if the particles are pulled apart or squashed together that energy is stored in the spring. Similarly there is potential energy between the particles in a substance.

21. Internal Energy The internal energy of a substance can be changed by heating it (or taking heat from it) or by doing work on the object (or having the object do work).

22. Heat transfer Conduction, convection and radiation. I’m not going to say anything about these, you should know it already. Can you construct a heat transfer mind- map?

23. Mind-map

24. Who is Mr Porter? Mr Porter

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36. Heat transfer Conduction, convection and radiation. I’m not going to say anything about these, you should know it already. Can you construct a heat transfer mind- map? Colours Few words Connections Drawings

37. Measuring temperature practical

38. Moles! Hi Chris!

39. Moles! Equal masses of different elements will contain different numbers of atoms (as atoms of different elements have different masses)

40. Moles! It is sometimes useful for physicists and chemists (but we don’t care about them) to compare the number of atoms or molecules in an amount of substance. To do this we use the idea of moles. A chemist

41. Moles! One mole of a substance contains the same number of molecules/atoms as in 12 grams of carbon-12. This number (of atoms or molecules) is known as the Avogadro constant (N A ) which is equal to 6.02 x 10 23 You need to learn this definition.

42. How big is 6 x 10 23 ? Imagine the whole of the United states You are here!

43. How big is 6 x 10 23 ? Imagine the whole of the United states covered in unpopped popcorn

44. How big is 6 x 10 23 ? Imagine the whole of the United states covered in unpopped popcorn to a depth of six miles!

45. How big is 6 x 10 23 ? Imagine the whole of the United states covered in unpopped popcorn to a depth of six miles! Count the grains and that is 6 x 10 23 ! 600000000000000000000000

46. Moles! For example, Hydrogen (H 2 ) has a relative molecular mass of 2, so 2 grams of hydrogen (one mole) contains the same number of molecules as atoms in 12g of carbon-12 (6.02 x 10 23 )

47. Moles! It follows therefore that 7g of lithium (atomic mass 7), 20g neon (atomic mass 20) or 39 g potassium (atomic mass 39) all contain the same number of atoms (1 mole or 6.02 x 10 23 atoms)

48. Moles! The number of moles of a substance can thus be found by dividing the mass of substance by its relative atomic or molecular mass n = mass/RAM

49. Example How many moles of sulphur atoms are there in 80g of sulphur? How many grams of carbon would have the same number of atoms?

50. Example How many moles of sulphur atoms are there in 80g of sulphur? How many grams of carbon would have the same number of atoms? N = mass/RAM = 80/32 = 2.5 moles

51. Example How many moles of sulphur atoms are there in 80g of sulphur? How many grams of carbon would have the same number of atoms? N = mass/RAM = 80/32 = 2.5 moles Mass of carbon = RAM x n = 12 x 2.5 = 30 g

52. Relative formula mass We can use the idea of moles and apply it to molecules using relative formula mass. C 2 H 5 OH RFM = (2 x 12) + (6 x 1) + (1 x 16) = 46 46g of ethanol = I mole of ethanol molecules

53. What about moles and gases?

54. Equal volumes Luckily, equal volumes of gas contain the same number of particles (at the same temperature and pressure)

55. Equal volumes For example, 1 litre of nitrogen contains the same number of molecules as there are atoms in one litre of Argon. A litre is 1000 cm 3 or 1 dm 3

56. Mole of gas One mole of any gas occupies 24 dm 3 (24000 cm 3 ) at standard temperature and pressure (25°C and 1 atmosphere) You will be given this in a question

57. Moles of gas = volume (cm 3 )/24000 = volume (dm 3 )/24 Learn this!

58. Let’s try some questions: Pages 161 and 162 Questions 1, 2, 4, 5 and 6

59. Don’t forget to read the relevant pages in your textbook (Pages 158-162)