Heat of Fusion Lab
Essay by EvanRay • August 10, 2015 • Lab Report • 668 Words (3 Pages) • 1,679 Views
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:
- 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)
- Pour water into the coffee cup calorimeter.
- Record the temperature in Celsius.
- Add a quantity of ice. (DO NOT EAT THE ICE!!!)
- Stir consistently and record this temperature when it stops dropping.Add more ice as necessary.
- Removes excessive ice with plastic spoon.
- Pour out water into a graduated cylinder to record the water that remains in mL and grams.
- Calculate Q using q=MC∆T equation
- Using the rearrange formula to solve for Hf.
Data Table | |
Amount of HOT water (mL) poured into calorimeter | 94 mL |
Mass of HOT water in calorimeter | 94g |
Temperature of HOT water. (Ti) | 64o C |
Temperature of water after Ice. (Tf) | 0o C |
∆T = (Tf – Ti) | -64o C |
Amount of water after Ice. (mL) | 175 mL |
Mass of water after Ice. | 175g |
Heat (Q) | -25170.94 Joules |
Hf | -310.75 J/g |
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.
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