Name _________________________________________ Period ______ Date __________________

Partner ________________________________________

HEAT OF FUSION OF ICEDATA:

V1 = _____________________ T1 = _____________________

V2 = _____________________ T2 = _____________________

CALCULATIONS (put a box around all answers):1. Using the density of water, find the mass (m1) of the original volume of water (V1).

D = 1.000 g/mL

2. Find the change in volume of water resulting from the melted ice. (ΔV = V2 - V1)

3. Find the mass (m2) of this change in volume of water, (ΔV). Make sure you use ΔV.

4. Find the change in the temperature of the water. (∆T = T1 - T2)

5. Find the heat lost by the original mass of water. (Q = m1 ∆T Cp)

6. Find the heat of fusion of ice. ΔHfus = Q m2

7. Find your percent error. The true value for the heat of fusion of ice is 334 J/g.

% error = (experimental value-true value) x 100 true value

CONCLUSIONS:1. List at least two possible sources of error in this experiment. (List things that actually could have

gone wrong – do not tell me you spilled water if you didn’t!) How might the use of a real calorimeter as one described in the background information reduce some of these errors?

EXTENSION AND APPLICATION:2. When is ice always 0°C?

3. What is dry ice? How is dry ice different from water ice (and we know they are different substances)?