Heat of Fusion Lab

Evan Ray Embrado

Mr. Coloumbe

Chem. Honors Per.4

April 28, 2015

Heat of Fusion of Ice (q=mHf)

Claim to Address:

How much heat does it take to change 1g of water from a solid to a liquid at 0o degrees Celsius?

As a chemist, your job is to find heat (Q) absorbed by a solid water (ice) in calories or Joules (This will be your numerator). Q (heat) will be divided by the total mass amount of ice that melts (g).

Procedures:

1. Pour between 50mL and 100 mL of hot water into a plastic graduated cylinder. Record this amount. (Useful information: the number recorded also represents the mass of the hot water density H20=1g/mL)
2. Pour water into the coffee cup calorimeter.
3. Record the temperature in Celsius.
4. Add a quantity of ice. (DO NOT EAT THE ICE!!!)
5. Stir consistently and record this temperature when it stops dropping.Add more ice as necessary.
6. Removes excessive ice with plastic spoon.
7. Pour out water into a graduated cylinder to record the water that remains in mL and grams.
8. Calculate Q using q=MC∆T equation
9. Using the rearrange formula to solve for Hf.

Claim: What is the Heat of Fusion of Ice

- The Heat of Fusion of ice is -310.75 J/g.

Evidence: is in your data table. Show all calculations used to support your claim. Include units.

Reason: Explain how and why your calculations represent the Heat of Fusion. Explain the sign for the Heat of Fusion and relate the phase diagram to the Heat of Fusion.

...