1. Challenge: To determine the melting point of water.
Your write up should include the following components:
I. TITLE
II. PURPOSE
MATERIALS-
IV. PROCEDURE
V. DATA
VI. CALCULATIONS/GRAPH
VII.CONCLUSION (including a discussion of sources of error.)

2. Vocabulary condensation temperature deposition vaporization freezing
Solidification
fusion
Crystallization
gaseous phase
melting
heat
solid phase
heat of fusion
liquid phase
heat of vaporization
sublimation

3. Types of energy
POTENTIAL ENERGY :
STORED ENERGY. The energy inside the substance.
KINETIC ENERGY : Associated with motion.
Average KE = TEMPERATURE

4. HEAT OF FUSION FOR WATER (TABLE B)
Amount of heat needed to completely melt 1g of water (ice!).
334 J/g
334 Joules of heat are necessary to completely melt 1 g of water.
HOW MUCH HEAT IS NEEDED TO MELT 10 g OF WATER?

5. HEAT OF VAPORIZATION FOR WATER (TABLE T)
The amount of heat needed to completely vaporize one g of water at its boiling point.
2260 J/g
Water needs 2260 J of heat per gram to convert to gas!

6. Summarizing
When there is a change in temperature use Q = m x C x T While the substance is melting/freezing use Q = m x H f While the substance is boiling/condensing use Q = m x H vap

7. Do now!
How much heat is needed to completely melt 10 g of ice at 0 0 C ?
How much heat is needed to vaporize 10 g of water at C ?

8. Energy Changes Associated with Changes of State
The heat added to the system at the melting and boiling points goes into pulling the molecules farther apart from each other.
The temperature of the substance does not change during a phase change !!!

9. Objectives Describe what happens with PE and KE as phase changes
Identify MP and BP from heating curve
MP=FP and BP=condensation point
Calculate the Hfus and Hvap from the heating curves
Cooling curves

10. Objective: How to calculate heat from heating curves
Do now: Draw a heating curve for the heating of 2 grams of substance that are being heated at a rate of 50 J/min. Melting Point 20 C Boiling Point 80 C Substance begins to melt at minute 2 and melts for 1 minute. It begins to boil at minute 8 and it takes 3 minutes to completely boil.

11. Endothermic Phase Changes
If the substance is melting or boiling, heat is being absorbed, and is being used to change the state of matter.
DURING THE PHASE CHANGE THE AVERAGE KINETIC ENERGY DOES NOT CHANGE!!! THE POTENTIAL ENERGY INCREASES.

12. Melting Point and Freezing Point
The temperature at which a substance melts. Is the same temperature at which the substance freeze.
Boiling Point and Condensation Point are the same temperature.
Normal boiling point is the temperature at which a liquid boils at normal pressure.

13. Exothermic changes
If the substance is undergoing condensation or freezing then heat energy is being released. The potential energy is decreasing and the TEMPERATURE REMAINS CONSTANT!!!

14. Objective: How to represent heat changes
Do now: Draw a cooling curve for the heating of 50 grams of substance that are being heated at a rate of 200 J/min. At minute 0 the substance is a gas. Substance begins to condense at minute 2 and it takes 7 minutes to turn completely to liquid at 70C. At minute 16 it begins to freeze and it takes 3 minutes till it solidifies completely at 20 C. Indicate Boiling Point, Melting Point and calculate heat of fusion and heat of vaporization.

15. VAPORIZATION IS ENDOTHERMIC
In hot climates drinking water is cooled by evaporating water from the surfaces of porous clay pots. As water evaporates it ABSORBS heat from the water inside the container which is maintained cool.
Like cooling yourself off on a hot day by pouring water over your body. As water evaporates it absorbs heat

18. FREEZING IS EXOTHERMIC
In freezing weather, citrus crops are sprayed with water to protect the fruit from frost damage. As the water freezes (around the fruit-outside the fruit!) it releases heat, which helps to prevent the fruit from freezing.

20. How to calculate the amount of heat that a substance absorbs while it is being heated up.
DO NOW
1 .-Calculate the amount of heat needed to increase the temperature of 200g of water from 0 0C to 100 0C. The heating rate is 100J/min.
2.-How much heat is needed to completely vaporize 200 g of water at 100 0C

21. Heating curve Homework answers
b and d
KE (temperature) remains constant
PE increases
3) S and L
4) 20 C
5) 60 C
6) Gas
7) Increases (is T!)
8) E

22. TOPICS FOR TEST TEMPERATURE SCALES/CONVERSIONS HEAT TRANSFER
CALORIMETRY PROBLEMS
SPECIFIC HEAT
PHASES OF MATTER
HEAT OF VAPORIZATION AND HEAT OF FUSION
ENDO AND EXO CHANGES
HEATING AND COOLING CURVES
BRING PENCIL AND REFERENCE TABLES
AND CALCULATOR!!!!!

23. HEATING/COOLING CURVE WORKSHEET ANSWERS
BC AND DE
AB, CD AND EF
9min x 60 kJ/min= 540kJ
7minx 60kJ/min= 420 kJ
24minx60kJ/min = 140 kJ
8minx60kJ/min=480kJ
Hvap= 480kJ/10kg
Hvap=48J/g AB CD EF DE

24. HEAT PRACTICE QUESTIONS (6163)B C A B C D

25. THE ROLE OF ENERGY IN CHANGES OF PHASE ANSWERS (Fill in)
ABSORPTION (ADDITION)
MELTING
BOILING
TEMPERATURE
KINETIC
MOLECULES
POTENTIAL
HEAT
KINETIC
POTENTIAL
COOLING
DECREASE
DECREASING

26. How to calculate heat from heating curves
9) Use information in the heading of the problem Mass of substance= Heating rate= 100 Joule/minute
20minx100J/min=2000J
2000J/20 g = 100J/g
1000J/20 g = 50 J/g
60 C

27. Twenty grams of a solid substance is heated starting from a temperature below its melting point at a constant rate of a 100 joule/minute.

28. Heat Answers
SET 2
13 3
14 4
15 4
16 3
17 3
18 2
19 2
20 3
J/g x 7.5 g= 915 J
SET 1 4 1 2 3

29. q (amount of heat ) table T
q = m C D T while T is changing (one phase)
q = m x Hfus during melting (2 phases- T constant )
q = m x Hvap during boiling (2 phases- T constant )

30. Heat of Fusion Hfus
Amount of heat needed to completely melt 1 gram of substance at its melting point. At the melting point the heat is calculated Heat = m x Hfus

31. Heat of Vaporization
Amount of heat needed to completely boil off 1 gram of substance at its boiling point.
At the boiling point the heat is calculated
Heat = m x Hvap