Homework Pg. 1087 #28,29,30,31,32 & Pg. 1112 #65,67,68

Homework Pg.1077 #22-26

Calculating Solubility

Pg. 1062 #1,2 Pg. 1068 #10,11 Pg. 1069 #12,13 Pg.1072 #14,15

Blog Homework Molarity Problems

Energy Specific Heat Worksheets

Enthalpy Worksheet

Calorimetry Worksheet

Entropy Worksheet #2

Entropy Worksheet #1

Homework Pg. 1176 #38,40

Candle Lab

Homework Pg.1189 #66

Homework Pg 1158 #24,25

Heat of Fusion Lab

                                                          Heat of Fusion for Ice

Purpose: The purpose is to find the heat of fusion for ice.

Procedure: 

1. Start with 100 ml H2O @ 50° Celsius.

2. Place into calorimeter and record the temperature.

3. Drop 2 to 3 ice cubes in and stir until temperature no longer drops. Remove any ice. Don't run out of ice. 

4. Measure new volume.

Data:

Starting Volume & Temperature: 100 ml of water---> 50° Celsius 

New Volume & Temperature: 163 ml of water---> 1.4° Celsius

Calculations: 

1. Mass of H2O used (100 ml = 100 g)

2. Find heat of hot H2O (m x delta T x c): 100x-48.7x4.18=-20356.6

3. Determine q ice: 100x48.7x4.18=20356.6

4. Determine mass of melted ice, then change to mols: 63 g--->3.5 mols (63/18=3.5)

5. Calculate delta H fusion (kJ/mol): 6.01 kJ/mol

Q heat = 163 ml

50 - 1.4 = 48.6

20356.6 J--->20.3kJ (a kilojoule is a hundredth of a joule, so when you move the decimal to one hundredth of a place, 20356.6J turns into 20.3kJ)

Conclusion: When ice is placed in hot water it will melt, but will not get colder past a certain temperature. The temperature of this certain point is 1.40° Celsius. This is because in a phase diagram, each section has its own specific temperature and pressure.