Mr. O
Lab 18 Calorimetry
Name:
Heat of fusion of ice
Pre-Lab Discussion:
Calorimeter is an insulated container made up of two chambers. The outer chamber
contains a known water mass. The inner chamber, the experimenter places the materials
that are to lose or gain heat while undergoing physical or chemical change. The transfer
of heat between the two chambers allows the experimenter to take a direct temperature
reading. Using the following formula the individual can calculate heat gained or lost.
Heat = mass of water x specific heat of water x change in temperature (q=mC T)
Equipment: 250 beaker, graduated cylinder, Styrofoam cup, thermometer, burner, ring
stand, iron gauze, tongs, and safety goggles.
Materials: water and ice
Observation and Data
V1=___________ V2=____________ T1=___________ T2=__________
Calculations:
1. Using the known density of water, find the mass(m1) of the original volume of
water.
2. Find the volume of water resulting from the melted ice. (V=V2 – V1)
3. Find the mass (m2) of the volume of water.
4. Find the change in temperature of the water.
T=T1 – T2)
5. Find the heat lost by the original mass of the water. ( q = m1 x C x T)
6. Find the heat of fusion of ice. ( q/m2)
7. Find your percent error. (true value of fusion 334 J/g)
Conclusion and Questions:
1. List the possible sources of error. How might the use of a calorimeter reduce
error?
2. One source of error is the flow of heat between the water in the cup and the
surroundings. Explain how this error is reduced by starting with water at about 50
degrees Celsius?
3. In what way does calorimetry make the use of the law of conservation of energy?
4. Define: exothermic, endothermic, heat of fusion, and specific heat capacity.
5. Is the process of melting exothermic or endothermic? Explain?
6. What is the difference between heat and temperature?