1. Can you stick the sheet in please?
Cool wax!
Can you stick the sheet in please?

2. Sketch a predicted graph
Temp (°C)
water ?
wax
Time (mins)

3. Today’s lesson
Describe melting and boiling in terms of energy input without a change of temperature
Distinguish between boiling and evaporation
Describe condensation and solidification
State the meaning of melting point and boiling point
Use the terms latent heat of vaporisation and latent heat of fusion and give a molecular interpretation of latent heat

4. Solids, liquids and gases

5. Cooling!

6. Latent heat
When pure substances cool, the temperature stops changing as the substance changes from a liquid to a solid.
Temp (°C)
Time (mins)
Melting point

7. Latent heat (“latent” = “hidden”)
When the molecules of a substance settle into the regular pattern of a solid, energy is released as bonds are formed. This energy released is called latent heat. This stops the temperature from falling.
(“latent” = “hidden”)

8. Latent heat
The opposite happens when a solid makes. Heat is needed to break the bonds between the solid particles (increasing their potential energy instead of raising the temperature (kinetic energy))
liquid
Melting point
Temp (°C)
solid
Time (mins)

9. The same happens when boiling

10. Specific Latent heat
The specific latent heat of a substance tells us how much energy is needed to change the state of 1 kg of substance at constant temperature.
Solid to liquid/liquid to solid or
liquid to gas/gas to liquid

11. Energy = mass x specific latent heat
Another formula!
Energy = mass x specific latent heat
E = mL

12. Specific Latent Heat
The specific latent heat of fusion (melting) of ice at 0 ºC, for example, is J/kg. This means that to convert 1 kg of ice at 0 ºC to 1 kg of water at 0 ºC, J of heat must be absorbed by the ice.
All at 0°C
1 kg
1 kg
J absorbed

13. Specific Latent Heat
Conversely, when 1 kg of water at 0 ºC freezes to give 1 kg of ice at 0 ºC, J of heat will be released to the surroundings.
All at 0°C
1 kg
1 kg
J released

14. Specific Latent Heat of Vaporisation
For water at its normal boiling point of 100 ºC, the latent specific latent heat of vaporization is J/kg. This means that to convert 1 kg of water at 100 ºC to 1 kg of steam at 100 ºC, J of heat must be absorbed by the water.
All at 100°C
1 kg
1 kg
J input

15. Latent heat
Conversely, when 1 kg of steam at 100 ºC condenses to give 1 kg of water at 100 ºC, 2260 kJ of heat will be released to the surroundings.
All at 100°C
1 kg
1 kg
J released

16. Example
The specific latent heat of fusion (melting) of ice is J/kg. How much energy is needed to melt 5kg of ice at 0°C to 5 kg of water at 0°C?
Energy = mL = 5 x = J

17. IB level calculation
Calculate the amount of heat required to completely convert 50 g of ice at 0 ºC to steam at 100 ºC. The specific heat capacity of water is 4.18 kJ/kg/°C. The specific latent heat of fusion of ice is 334 kJ/kg, and the specific heat of vaporization of water is 2260 kJ/kg.
50g
0°C
50g
100°C

18. An example calculation
Heat is taken up in three stages:
1. The melting of the ice.
2. The heating of the water.
3. The vaporization of the water.
0°C
0°C
100°C
100°C

19. Stage 1 1. Heat taken up for converting ice at 0ºC to water at 0ºC
mass of water x latent heat of fusion = (kg) x 334 (kJ.kg-1) = 16.7 kJ
0°C

20. Stage 2
2. Heat taken up heating the water from 0 ºC to the boiling point, 100 ºC
mass of water x specific heat capacity x temperature change = 0.05 (kg) x 4.18 (kJ.kg-1.°C-1)x 100 (ºC) = 20.9 kJ
0°C
100°C

21. Stage 3 3. Heat taken up vaporising the water
mass of water x latent heat of vaporization 0.05 (kg) x 2260 kJ.kg-1 = 113 kJ
100°C

22. The answer
The sum of these is
= kJ (151 kJ)

23. Got it?

24. Just time for a quick dog accident
50 kg
Just time for a quick dog accident

25. Ooops!
50 kg

26. Let’s try some questions

27. Boiling and evaporation

28. Evaporation
Consider a beaker of water at room temperature

29. Evaporation
The molecules of water are moving around at different speeds, some fast, some slow.
# of molecules at a particular speed
speed of molecule (m/s)
Average speed

30. Evaporation
If a molecule is at the surface, and moving fast enough, it may escape the liquid. This is called evaporation.
Freedom!

31. Evaporation
Since the average speed of the remaining molecules must now be lower, the temperature of the liquid drops (since temperature is a measure of the kinetic energy of the molecules). To gain the additional energy necessary to break free, the individual molecule must steal heat energy from neighbors.
Freedom!

32. Evaporation
Evaporation can thus take place at any temperature.

33. Boiling? 33

34. Boiling
Boiling occurs when vapour is produced in the body of the liquid.
What’s in the bubbles?

35. Boiling
Boiling occurs when vapour is produced in the body of the liquid.
The bubble contains only water vapour, not air!

36. Boiling
Boiling occurs when vapour is produced in the body of the liquid. This only happens at the boiling point of the liquid.
The bubble contains only water vapour, not air!

37. To summarize:
Evaporation takes place only at the surface of the liquid and can take place at any temperature.

38. To summarize:
Boiling means bubbles!
Boiling occurs when vapour is produced in the body of the liquid. This only happens at the boiling point of the liquid.

39. OK, now try to answer some questions!
Page 115 Q 5
Page 119 Qs 1, 2, 3, 4.