PASCO TD-8557 User manual

®Instruction Manual and
Experiment Guide
012-03060D
Basic Calorimetry Set
TD-8557
CALORIMETER
MAX TEMP: 100°C
P/N: 650-02975
Al
Cu
Pb

®
Table of Contents
ii
Introduction . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 1
Notes on Calorimetry. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 2
Experiment 1: What is a Calorie? . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 3
Experiment 2: Specific Heat . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 5
Experiment 3: Latent Heat of Vaporization . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 8
Experiment 4: Latent Heat of Fusion . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 10

Basic Calorimetry Set
TD-8557
®1
Included Parts
1. Calorimeters, 6 pieces
2. Water trap with plastic tubing
3. Aluminum sample
4. Copper sample
5. Lead sample
6. Thermometer
Introduction
Understanding calorimetry is the first step into the field of thermodynamics, the study of the role of heat in physical
processes. With the addition of a balance, ice, and a heat source, such as PASCO’s Model TD-8556 Steam Generator,
this Basic Calorimetry Set provides the equipment necessary to perform a variety of calorimetry experiments. Four
important, introductory experiments are described in this manual:
Experiment 1: What is a Calorie? An introduction to the ideas of temperature and heat, and a demonstration
of the conservation of energy.
Experiment 2: Thermal Capacity and Specific Heat The specific heats of aluminum, copper, and lead are
measured.
Experiment 3: Latent Heat of Vaporization The role of heat transfer in the conversion of steam into water is
investigated.
Experiment 4: Latent Heat of Fusion The role of heat transfer in the conversion of ice into water is investi-
gated.
CALORIMETER
MAX TEMP: 100°C
P/N: 650-02975
2
345
6
1

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Notes on Calorimetry
A calorimeter is a vessel or device that thermally isolates an experiment from its surround-
ings. Ideally, this means that the results of an experiment performed in a calorimeter are
independent of the temperature of the surroundings, because no heat flows into or out of
the calorimeter.
However, no calorimeter is perfect, and there is always some unwanted and unaccountable
heat flow affecting the results of any calorimetric experiment. To minimize unwanted heat
flow, always plan the experiment to follow these rules:
1. The time between the taking of initial and final temperatures is minimal.
In other words, do the critical portion of the experiment quickly, so there is minimal time
for unwanted heat flow between measurements. (Don’t rush; just plan carefully.)
2. Whenever possible, room temperature is approximately midway between
the beginning and ending temperatures of the experiment. When the experi-
mental temperature is colder than room temperature, heat flows from the surroundings
into the calorimeter. When the experimental temperature is hotter than room temperature,
heat flows from the calorimeter into the surroundings. If the experimental temperature
varies above and below room temperature by equal amounts, the heat gained and lost to
the environment will be approximately equal, minimizing the net affect on the experiment.
3. Mass measurements of liquids are made as near the critical temperature
measurements as possible. This reduces the effects of mass loss by evaporation.
Measuring liquid masses by taking appropriate differences is a useful technique (see the
instructions in the individual experiments).
NOTE: In applying the above rules, it is often helpful to perform a quick preliminary experiment to
determine the best choice for initial masses and temperatures.

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Experiment 1: What is a Calorie?
Equipment Needed
• Calorimeters, 2 pieces
• Thermometer
• Balance
• Hot and cold water
Introduction
When two systems or objects of different temperature come into contact, energy in the
form of heat is transferred from the warmer system into the cooler. This transfer of heat
raises the temperature of the cooler system and lowers the temperature of the warmer sys-
tem. Eventually the two systems reach some common, intermediate temperature, and the
heat transfer stops.
The standard unit for measuring heat transfer is the calorie. A calorie is defined as the
amount of energy required to raise the temperature of one gram of water from 14.5° C to
15.5° C. However, for our purposes, we can generalize this definition by simply saying
that a calorie is the amount of energy required to raise the temperature of one gram of
water one degree Celsius (the variation with temperature is slight).
In this experiment, you will combine hot and cold water of known temperature and mass.
Using the definition of the calorie, you will be able to determine the amount of heat energy
that is transferred in bringing the hot and cold water to their final common temperature,
and thereby determine if heat energy is conserved in this process.
Procedure
1. Determine the mass of the empty calorimeter, Mcal. Record your result in Table 1.1.
2. Fill the calorimeter about 1/3 full with cold water. Measure the mass of the calorime-
ter and water together to determine Mcal + water cold. Record your result.
3. Fill a second calorimeter approximately 1/3 full of hot water. The water should be at
least 20° C above room temperature. Weigh the calorimeter and water together to
determine Mcal + water hot. Record your result
4. Measure Thot and Tcold, the temperatures the hot and cold water, and record your
results.
5. Immediately after measuring the temperatures, add the hot water to the cold water and
stir with the thermometer until the temperature stabilizes. Record the final tempera-
ture of the mixture, Tfinal.
6. Measure the final mass of the calorimeter and mixed water, Mfinal.
7. Repeat the procedure twice with different masses of water at different temperatures.
(You might try adding cold water to hot instead of hot to cold.)

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Data
Calculations
From your data, make the calculations necessary to determine the mass of the cold and hot
water (Mwater cold and Mwater hot), and also the temperature changes undergone by each
(∆Tcold and ∆Thot). Enter your results in Table 1.2.
Using the equations shown below, calculate ∆Hcold and ∆Hhot, the heat gained by the cold
and hot water, respectively. Enter your results in the table.
∆Hcold = (Mwater cold)(∆Tcold)(1 cal/g K)
∆Hhot = (Mwater hot)(∆Thot)(1 cal/g K)
Questions
1. Which had more thermal energy, the two cups of water before they were mixed
together or after they were mixed? Was energy conserved?
2. Discuss any unwanted sources of heat loss or gain that might have had an effect on
the experiment.
3. If 200 g of water at 85° C were added to 150 g of water at 15° C, what would be the
final equilibrium temperature of the mixture?
Table 1.1: Data
Trial 1 Trial 2 Trial 3
Mcal
Mcal + water cold
Mcal + water hot
Tcold
Thot
Tfinal
Mfinal
Table 1.2: Calculations
Trial 1 Trial 2 Trial 3
Mwater cold
Mwater hot
∆Tcold
∆Thot
∆Hcold
∆Hhot

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Experiment 2: Specific Heat
Equipment Needed
• Calorimeter
• Thermometer
• Samples of aluminum, copper, and lead
• Balance
• Boiling water
• Cool water
• Thread
• Antifreeze, approximately 100 g
Introduction
The Specific Heat of a substance, usually indicated by the symbol c, is the amount of heat
required to raise the temperature of one gram of the substance by 1° C (or 1 K). From the
definition of the calorie given in Experiment 1, it can be seen that the specific heat of
water is 1.0 cal/g K. If an object is made of a substance with specific heat equal to csub,
then the heat, ∆H, required to raise the temperature of that object by an amount ∆Tis:
∆H= (mass of object) (csub) (∆T)
In Part 1 of this experiment you will measure the specific heats of aluminum, copper, and
lead. In Part 2 you will measure the specific heat of antifreeze.
CAUTION: This experiment involves the use of boiling water and the handling of HOT metal
objects. Work carefully.
Part 1: The Specific Heats of Aluminum, Copper, and Lead
1. Measure Mcal, the mass of the calorimeter you will use (it should be empty and dry).
Record your result in Table 2.1.
2. Measure the masses of the aluminum, copper, and lead samples. Record these masses
in Table 2.1 in the row labeled Msample.
3. Attach a thread to each of the metal samples and suspend each of the samples in boil-
ing water. Allow a few minutes for the samples to heat thoroughly.
4. Fill the calorimeter approximately 1/2 full of cool water—use enough water to fully
cover any one of the metal samples.
5. Measure Tcool, the temperature of the cool water. Record your measurement in the
table.
6. Immediately following your temperature measurement, remove one of the metal sam-
ples from the boiling water, quickly wipe it dry, then suspend it in the cool water in
the calorimeter (the sample should be completely covered but should not touch the
bottom of the calorimeter).
7. Stir the water with the thermometer and record Tfinal, the highest temperature attained
by the water as it comes into thermal equilibrium with the metal sample.
8. Immediately after taking the temperature, measure and record Mtotal, the total mass of
the calorimeter, water, and metal sample.

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Part 2: The Specific Heat of Antifreeze
Repeat Part 1 of this experiment, but instead of using the metal samples, heat approxi-
mately 100 g of antifreeze to approximately 60° C. Measure and record the temperature,
then quickly pour the antifreeze into a calorimeter containing cool water and stir until the
highest stable temperature is reached (about 1 minute). Record your data and calculations
on a separate sheet of paper. You will need the following data:
•Mcal, the mass of the calorimeter,
•Mwater the mass of the calorimeter plus water,
•Tcool the temperature of the cool water,
•Mtotal, the mass of the calorimeter plus water plus antifreeze
•Tfinal, the temperature of the water plus antifreeze.
Data and Calculations
Part 1
For each metal tested, use the equations shown below to determine Mwater, the mass of the
water used, ∆Twater, the temperature change of the water when it came into contact with
the metal sample, and ∆Tsample, the temperature change of the metal sample when it came
into contact with the water. Record your results in Table 2.1.
Mwater = Mtotal - (Mcal + Msample)
∆Twater = Tfinal - Tcool
∆Tsample = 100° C - Tfinal
From the law of energy conservation, the heat lost by the metal sample must equal the heat
gained by the water:
Heat lost by sample = (Msample) (csample) (∆Tsample) = (Mwater) (cwater) (∆Twater) = Heat gained by water
cwater is the specific heat of water, which is 1.0 cal/g K.
Use the above equation, and your collected data, to solve for the specific heats of alumi-
num, copper, and lead. Record your results in the bottom row of Table 2.1.
Table 2.1: Data and Calculations (Part 1)
Trial 1 Trial 2 Trial 3
Mcal
Msample
Tcool
Tfinal
Mtotal
Mwater
∆Twater
∆Tsample
c

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Part 2
Mcal = ____________
Mwater = ____________
Tcool = ____________
Mtotal = ____________
Tfinal = ____________
Perform calculations similar to those performed in part 1 to determine cantifreeze, the spe-
cific heat of antifreeze.
cantifreeze = ____________
Questions
1. How do the specific heats of the samples compare with the specific heat of water?
2. Discuss any unwanted heat loss or gain that might have effected your results?
3. From your measured specific heat for antifreeze, which should be the better coolant
for an automobile engine, antifreeze or water? Why is antifreeze used as an engine
coolant?

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Experiment 3: Latent Heat of Vaporization
Equipment Needed
• Calorimeter
• Thermometer
• Steam Generator
• Water Trap
•Tubing
• Balance
If a steam generator is not available, a distillation flask and
Bunsen burner is adequate. A second flask can be used as a
water trap.
Introduction
When a substance changes phase, the arrangement of
its molecules changes. If the new arrangement has a
higher internal energy, the substance must absorb heat
in order to make the phase transition. Conversely, if
the new arrangement has a lower internal energy, heat
will be released as the transition occurs.
In this experiment you will determine how much
more energy is contained in one gram of steam at
100°C, than in one gram of water at the same temperature. This value is called the Latent
Heat of Vaporization of water.
CAUTION: This experiment involves the use of boiling water and steam. Work carefully.
Procedure
1. Measure Trm, the room temperature.
2. Set up a steam generator with a water trap as shown in Figure 3.1. The tube lengths
should be approximately as shown in the figure.
3. Determine Mcal, the mass of a the empty, dry calorimeter.
4. Fill the calorimeter approximately 1/2 full of cool water about 10° C below room
temperature.
5. Turn on the steam generator and wait for the steam to flow freely for at least a minute.
6. Measure Tinitial and Mcal + water, the temperature of the cool water and the mass of the
water plus calorimeter.
7. Immediately immerse the free end of the short tube into the cool water in the calorim-
eter. Stir the water continuously with the thermometer.
IMPORTANT: The bottom of the water trap should be kept higher than the water level in the calorime-
ter to avoid water being pulled from the calorimeter back into the water trap.
8. When the water temperature, T, gets as far above room temperature as it was initially
below room temperature, remove the steam tube. Continue stirring the water and
record the highest stable temperature attained by the water (Tfinal).
CALORIMETER
MAX TEMP: 100°C
P/N: 650-02975
Figure 3.1: Equipment set-up
tubing, 25 cm tubing, 35 cm
glass tube to
restrict opening
water
trap
steam
generator

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IMPORTANT: Always remove the steam tube from the water before turning off the steam generator
heat. (Can you explain why?)
9. Immediately determine Mfinal, the mass of calorimeter plus water plus (condensed)
steam.
Data
Trm = ____________
Mcal = ____________
Tinitial = ____________
Mcal + water = ___________
Tfinal = ____________
Mfinal = ____________
Calculations
When steam condenses in cool water, heat energy is released into the water in two ways.
First, the latent heat of vaporization is released. With this release of heat, the steam is con-
verted into water, but the newly converted water is still at boiling temperature, 100° C.
Second, the newly converted water releases heat as it comes into thermal equilibrium with
the cooler water at a final equilibrium temperature, Tfinal.
According to the principle of the conservation of energy, the total heat released by the
steam equals the total heat absorbed by the cooler water. Stated mathematically:
(Msteam)(Hv) + (Msteam)(1 cal/g K)(Tsteam - Tfinal) = (Mwater)(1 cal/g K)(Tfinal - Tinitial)
Msteam = Mfinal - Mcal + water = __________________
Mwater = Mcal + water - Mcal = __________________
Tsteam = 100 °C
Hv= the latent heat of vaporization per gram of water
Use your data and the above information to determine Hv.
NOTE: The thermometer also absorbs a certain amount of heat during the experiment. As a good
approximation, assume that the heat capacity of the thermometer is equivalent to that of 1 g of water
(i.e., add 1 g to
M
water the above equation).
Hv= ____________
Questions
1. Why would an injury caused by 1 g of steam at 100° C do more damage than an in
jury caused by 1 g of water at 100° C?
2. Speculate on how the heat of vaporization might influence climate and weather sys-
tems.
3. In what way does water used to cook food serve as a refrigerant? (Hint: What happens
when the water all boils away?)

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Experiment 4: Latent Heat of Fusion
Equipment Needed
• Calorimeter
• Thermometer
• Ice in water (at melting point)
•Warmwater
Introduction
Just as steam has a higher internal energy content than water, so water has a higher internal
energy content than ice. It takes a certain amount of energy for the water molecules to
break free of the forces that hold them together in the crystalline formation of ice. This
same amount of energy is released when the water molecules come together and bond to
form the ice crystal.
In this experiment, you will measure the difference in internal energy between one gram
of ice at 0° C and one gram of water at 0° C. This difference in energy is called the latent
heat of fusion of water.
Procedure
1. Measure Trm, the room temperature.
2. Determine Mcal, the mass of the empty, dry calorimeter.
3. Fill the calorimeter approximately 1/2 full of warm water about 15° C above room
temperature.
4. Measure Mcal + water, the mass of the calorimeter and water.
5. Measure Tinitial, the initial temperature of the warm water.
6. Add small chunks of ice to the warm water, wiping the excess water from each piece
of ice immediately before adding. Add the ice slowly, stirring continuously with the
thermometer until each chunk melts.
7. When the temperature of the mixture is as much below room temperature as the warm
water was initially above room temperature and all the ice is melted, measure the final
temperature of the water (Tfinal).
8. Immediately after measuring Tfinal, weigh the calorimeter and water to determine
Mfinal.
Suggested Additional Experiment
Repeat the above experiment, but, instead of ordinary ice, use the material which is pack-
aged in metal or plastic containers to be frozen and used in picnic coolers.
Data
Trm = ________________
Mcal = ________________
Mcal + water = ________________
Tinitial = ________________

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Tfinal = ________________
Mfinal = ________________
Calculations
According to the principle of the conservation of energy, the quantity of heat absorbed by
the ice as it melts and then heats up to the final equilibrium temperature must equal the
quantity of heat released by the warm water as it cools down to the final equilibrium tem-
perature. Mathematically:
(Mice)(Hf) + (Mice)(1 cal/g K)(Tfinal - 0° C) = (Mwater)(1 cal/g K)(Tinitial - Tfinal)
Mice = Mfinal - Mcal + water = __________________
Use your data and the above information to determine Hf, the latent heat of fusion per
gram of water.
Hf= the latent heat of fusion per gram of water
Questions
1. What advantage might the commercially packaged coolant material have over ice
other than that it produces less mess? (If you didn’t perform the optional part of the
experiment, what properties would a material need in order to be a better coolant than
ice?)
2. Design an experiment to determine which of two substances (for instance, ice and
packaged coolant) will keep an insulated food cooler
a. cool for the longest time, and
b. at a lower temperature.

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For more information about the Basic Calorimetry Set and the latest revision of this Instruction Manual, visit:
www.pasco.com/go?TD-8557
Limited Warranty For a description of the product warranty, see the PASCO catalog. Copyright The PASCO scientific
012-03060D
Basic Calorimetry Set Instruction Manual is copyrighted with all rights reserved. Permission is granted to non-profit edu-
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