Fusion Report Sheet

Heat of Fusion Report Sheet

Data
Intial volume of water in the styrofoam cup (before the ice was added) (mL)
100
Final volume of water in the styrofoam cup (after the ice melted) (mL)
145
Volume of water due to melted ice (mL)

45
Mass (g) melted ice

45
Initial temperature (°C) of the water placed in the styrofoam cup
47.3
Minimum temperature (°C) after the ice was melted
45

Calculations
1. The amount of liquid water placed in the cup was _____100_______ mL. Assume that the density of water is 1.0 g/mL. What is the weight in grams of the liquid water?

Yes, because the density of water is 1

2. Calculate the temperature change.
47.3-4=43.5

3. Knowing that the specific heat of water is 4.184 J/g°C, calculate the total amount of heat released by the 100 ml of water as it cooled. This energy was used to melt the ice and then raise the temperature of the melted ice from 0 °C to the minimum temperature of the system.
Heat lost by liquid water = (mass)(specific heat)(∆T)

H=100x4.284x43.5=18200.4J

4.
The amount of heat lost by the liquid water was _______18200.4j_______. Assuming that the Law of Conservation of Energy applies, the amount of heat absorbed by the melting ice was ___________8660.52___.

5. Calculate the volume of water contributed to the cup by the melted ice.
145-100=45

6. Assume that the density of ice is 1.00 g/ml. Calculate the mass of ice melted.

45x1=45g

7. Calculate the heat of fusion of ice in J/g.

45x4.814x9x(-4)=8660.52

8. Convert the molar heat of fusion of ice from J/g to kJ/mole.

8.66

9. Calculate the % error. The accepted value for the molar heat of fusion of ice is 6.01 kJ/mole
75%

10. List three sources of error.

Human error, experiment, room temperature.