This document summarizes a practicum report on using a calorimeter to measure heat. The report details the purpose, theory, tools, steps, data, calculations, and discussion. The practicum aims to determine the type of calorimeter, amount of heat energy released, electrical energy received, and understand calorimeter material. Measurements are taken of the calorimeter's mass, temperature changes when electrical current is passed through. Calculations are done to find the heat, electrical energy, power, and verify the relationship between electrical and heat energy using a correlation factor.

1. PRACTICUM REPORT
BASIC PHYSICS1
"CALORIMETER"
COLLECTION DATE : NOVEMBER 20, 2017
PRACTICAL DATE : 28 NOVEMBER 2017
"CALORIMETER"
A. PRACTICUM PURPOSE
1. Can determine the type of calorimeter.
2. Can determine the amount of heat energy released by the calorimeter.
3. Can determine the amount of electrical energy received by the calorimeter.
4. Can understand calorimeter material.
5. Can determine the value of heat-electric equality in the calorimeter.
B. BASIC THEORY Thethe calorimeter is a device used to determine (measure) heat.
The measurement is done to find out the heat of a type of substance. If the heat of
a type of substance is known, the heat absorbed or released can be calculated by
measuring the change in temperature. Calorimeter consists of a metal vessel whose
heat of type has been previously known. The vessel is placed in another vessel
container separated (there is no possibility of direct contact) between the two
vessels given an insulator which prevents heat exchange from the outside air. If an
object releases heat, there will be a change in the form of the substance in addition
to a change in size. For example, water, is cooled will turn into ice. From the first
water in the form of liquid, it turns into ice. From liquid to solid. Similarly, what
happens to liquid objects that evaporate intoa gas (Purwoko, 2007).
The working principle of the calorimeter is based on the Black Principle which
is stated as follows:
If two objects that have different temperatures are brought close so that contact
occurs, the final temperature of the two objects that have different temperatures
after the thermic balance is reached will be the same.
The amount of heat received = the amount of heat given.
(Wahyuni, 2010).
There are several things related to heat, namely:

2. Heat type is the amount of heat needed to increase 1 gram or 1 kg of a substance by
1°C. Heat capacity is the amount of heat needed by a substance to increase its
temperature by 1°C. Heat melting, expressing the amount of heat needed by a unit
of mass of solids to convert all of its forms into liquid. Frozen heat is the amount of
heat released to convert 1 kg of substance from liquid to solid at its freezing point.
The normal melting point of a substance or particle can be known or determined by
the attraction between the particles in it. Steam heat is the amount of heat absorbed
to convert 1 kg of a substance from its liquid form to vapor at its boiling point. Dew
heat is the amount of heat released to change 1 kg of substance from the form of
steam to liquid at the dew point. The normal boiling point of a liquid is a case where
the liquid vapor pressure is equal to the pressure of the atmosphere on the sea
surface. (Sunaryono, 2010).
The calorimeter is a quantitative measurement of heat entering during a
chemical process. The calorimeter is a tool to measure the heat of a reaction issued.
Calorimeters can be used to calculate the energy in food in the atmosphere and
measure the amount of energy that increases in the calorimeter temperature
(Wahyu, 2010).
A substance when given a continuous heat and releases the maximum heat, then
the substance will undergo a change in form. This event also applies if a substance
releases heat continuously and reaches its minimum temperature. Therefore, other
than heat can be used to change the temperature of substances can also be used to
change the form of substances (Soedojo, 1999).
Measuring the amount of heat a reaction is absorbed or released in a chemical
reaction with an experiment is called a calorimeter. By using his law, the heat of
reaction of a chemical reaction can be determined based on data on enthalpy
changes. The standard formation, bond energy and experimentally. The process in
the calorimeter takes place adiabatically, ie there is no loose energy or entering from
the outside into the calorimeter, and the law that applies to this process is the black
principle, namely:
Qfreelance = Qaccept
Q = mc∆T
Description:
Q = number of heat ( joule)

3. M = mass of substance (gram)
C = heat of type (cal / groc)
∆T = temperature change
(Zemansky, 1988)
Before further being explained about the calorimeter, first recognize the terms
in the calorimeter as follows:
The heat of type of substance is the heat needed to increase the temperature of
one unit of mass of the substance by one degree. Heat capacity is the heat needed
to raise the temperature of all objects by one degree. Melting heat is the heat needed
to melt one unit of mass at a fixed temperature. Frozen heat is the heat released
when the substance freezes. Normal melting point is the point where the object
changes into a liquid. Steam heat is the amount of heat needed to evaporate a unit
of liquid mass at a fixed temperature. Dew heat is the amount of heat needed to
change form from gas to liquid one unit of liquid mass at a fixed temperature. The
normal boiling point is the temperature where the pressure of a liquid is the same
as the external pressure experienced by a liquid (Bueche, 2006).
If two systems with different temperatures are united, the last temperature
reached by the two systems is between these two surface temperatures. A material
substance, namely caloric, is contained in every object. An object at high
temperatures contains more calories than a low-temperature object. When the two
objects are put together, the object rich in calories loses some of the calories given
by the other body until the two objects have not reached the same temperature. The
caloric theory is able to explain the mixing of substances in a calorimeter. While
the calorimeter is a tool to determine the heat of a type of substance (Halliday,
1999).
C. TOOLS AND MATERIALS
NO PICTURES
NAME OF TOOLS AND
MATERIALS

4. 1 Digital Balance
2 Connecting Cable
3 Power Supply
4 Calorimeter
5 Neraca O'haus
6 Stopwatch
7 Thermometer

5. 8 Measuring Cup
9 Water
10 Digital Multimeters
D. WORK STEPS
NO PICTURES
NAME TOOLS AND
MATERIALS
1
Prepare a tool for calorimeter
practicum.
2
Measure the calorimeter mass
with a digital balance.
3 Add water to the calorimeter.

6. 4
Re-measure the calorimeter mass
that is filled with water.
5
Measure the initial temperature
on the calorimeter and record
the results.
6
Make a series on the
amperemeter, and parallel it to
the voltmeter, as well as set the
voltage on the voltmeter, and the
current on the ammeter.
7
Connect to the power and press
the power button and adjust the
voltage.
8
Stir the water in the calorimeter
for three minutes.
9
Look at the final temperature,
then look at the two multimeters
and turn off the power supply.
10
Record the data that has been
obtained from the lab.

7. E. EXPERIMENT DATA
No
.
(V)
Pow
er
sup
ply
mk
(kg)
ma (kg)
T0
(°C)
Tt
(°C)
∆𝑇
(oC
)
Voltage
(V)
I
(A)
t
(s)
1. 6
0.144
5
0.0824
5
27 29 2 5.59
0.8
5
18
0
2. 6
0.144
5
0.0845 27 31 4 5.6 1
18
0
3. 6 0.142
0.087O
F
27 31 4 5.6 1
18
0
F. MANAGEMENT DATA
Looking for Water Calories
1. :
ma = 0.08245 𝑘𝑔
𝑄 = 4200 J / kg °C
∆𝑇 = 2 °C
1 𝐽 = 0.24 𝑐𝑎𝑙
Dit:
𝑄 = 𝑚𝑐∆𝑇
𝑄 = (0.08245 𝑘𝑔) (4200 J /
kg °C) (2°C)
𝑄 = 692.58 J x 0.24
𝑄 = 166,2192 𝑐𝑎𝑙
2. Dik:
ma = 0.0845 𝑘𝑔
𝑄 = 4200 J / kg °C
∆𝑇 = 4 °C
1 𝐽 = 0.24 𝑐𝑎𝑙
Dit:
𝑄 = 𝑚𝑐∆𝑇
𝑄 = (0.0845 𝑘𝑔) (4200 J /
kg °C) (4°C)
𝑄 = 1419.6 J x 0.24
𝑄 = 340,704 𝑐𝑎𝑙
3. Dik:
ma = 0.0845 𝑘𝑔
𝑄 = 4200 J / kg °C
Looking for Electric Energy.
1. Dik:
𝑉 = 5.59 𝑉
𝐼 = 0.85 𝐴
𝑡 = 180 𝑠
Dit:
W = VIt
𝑊 = 𝑉𝐼𝑡
𝑊 = (5.59 𝑉) (0.85 𝐼)
(180 𝑠)
𝑊 = 855.27 J
2. Dik:
𝑉 = 5.60 𝑉
𝐼 = 1.00 𝐴
𝑡 = 180 𝑠
Dit:
W = VIt
𝑊 = 𝑉𝐼𝑡
𝑊 = (5.60 𝑉) (1.00 𝐼)
(180 𝑠)
𝑊 = 1008.0 J
3. Dik:
𝑉 = 5.60 𝑉
𝐼 = 1.00 𝐴
𝑡 = 180 𝑠
Dit:

8. ∆𝑇 = 4 °C
1 𝐽 = 0.24 𝑐𝑎𝑙
Dit:
𝑄 = 𝑚𝑐∆𝑇
𝑄 = (0.0845 𝑘𝑔) (4200 J /
kg °C) (4°C)
𝑄 = 1461.6 J x 0.24
𝑄 = 350,784 𝑐𝑎𝑙
Qtotal = 166,2192 + 340,704 + 350,784
Qaverage = 285,9024 ≈ 286 times.
Calculation of Electric Power.
1. Dik:
V = 5.59
I = 0.85
Dit:
P = VI
P = (5.59) (0.85)
P = 4.7515 Watt
2. Dik:
V = 5.6
I = 1
Dit:
P = VI
P = (5.6) (1)
P = 5.6 Watt
3. Dik:
V = 5.6
I = 1
Dit:
P = VI
P = (5.6) (1)
P = 5.6 Watt
Ptotal = 4,7515 + 5,6 + 5,6
Paverage = 5,3172 ≈ 5.3 Watts
Relationship between Electric
Energy and Heat Energy.
1. Dik:
ma = 82.45𝑔𝑟
𝐶 𝑎 = 1 cal / gr °C
𝐶 𝑘 = 0.217𝑘𝑎𝑙 / 𝑔𝑟 ° 𝐶
Mk = 144.5
W = VIt
𝑊 = 𝑉𝐼𝑡
𝑊 = (5.60 𝑉) (1.00 𝐼)
(180 𝑠)
𝑊 = 1008.0 J
Wtotal = 855.27 + 1008 + 1008
Waverage = 957.09 ≈ 957 A
Calculation of Electricity
Constraints.
1. Dik:
V = 5.59
I = 0.85
Dit:
R = V / I
R = (5.59) / (0.85)
R = 6.5764 Ω
2. Dik:
V = 5.6
I = 1
Dit:
R = V. / I
R = (5.6) / (1)
R = 5.6 Ω
3. Dik:
V = 5.6
I = 1
Dit:
R = V. / I
R = (5.6) / ( 1)
R = 5.6 Ω
Rtotal = 6.5764 + 5.6 + 5.6
Raverage = 5.9254esi ≈ 6
Correlation Factor Relations or heat
equality (𝛾) .
1. Dik:
W = 855.27 J
Q = 227.513 kal
Dit:
𝛾 =
𝑊
𝑄
𝛾 =
855.27
227,513

9. ∆𝑇 = 2 °C
Dit:
𝑄 = 𝑚𝑐∆𝑇
𝑄 = ((ma.Ca) + (mk.Ck)) ∆𝑇
𝑄 = ((82.4𝑥1) + (144,5𝑥0,217)2
𝑄 = (82.4 + 31,3565)2
𝑄 = 227,513 𝑡𝑖𝑚𝑒𝑠
2. Dik:
ma = 84,5𝑔𝑟
𝐶 𝑎 = 1 cal / gr °C
𝐶 𝑘 = 0,217𝑘𝑎𝑙 / 𝑔𝑟 ° 𝐶
Mk = 144.5
∆𝑇 = 4 °C
Dit:
𝑄 = 𝑚𝑐∆𝑇
𝑄 = ((ma.Ca) + (mk.Ck)) ∆𝑇
𝑄 = ((84,5𝑥1) + (144,5𝑥0,217)2
𝑄 = (84.5 + 31,3565)4
𝑄 = 463,426 𝑘𝑎𝑙
3. Dik:
ma = 87,0𝑔𝑟
𝐶 𝑎 = 1 cal / gr °C
𝐶 𝑘 = 0,217𝑘𝑎𝑙 / 𝑔𝑟 ° 𝐶
Mk = 142
∆𝑇 = 4 °C
Dit:
𝑄 = 𝑚𝑐∆𝑇
𝑄 = ((ma.Ca) + (mk.Ck)) ∆𝑇
𝑄 = ((87.0𝑥1) + (142𝑥0.217)2
𝑄 = (87 + 30,814)4
𝑄 = 471,256 𝑘𝑎𝑙
Rtotal = 227,513 + 463,426 + 471,256
Raverage = 387,3983 ≈ 387 cal
𝛾 = 3.7592
2. Dik:
W = 1008.0 J
Q = 463,426 kal
Dit:
𝛾 =
𝑊
𝑄
𝛾 =
1008
463,426
𝛾 = 2.1751
3. Dik:
W = 1008,0 J
Q = 471,256 kal
Dit:
𝛾 =
𝑊
𝑄
𝛾 =
1008
471,256
𝛾 = 2.1389
𝛾total = 3.7592 + 2.1751 + 2.1389
𝛾average = 2.6911 ≈ 3
G. DISCUSSION
In this practicum, the practitioner performs a practicum, namely a calorimeter.
Simply put is a tool for measuring heat but an energy exchange from the basic
technique known as calorimetry which is a measurement quantitative from heat
exchange. to make such measurements is a calorimeter used in simple water
calorimetry.

10. In this practicum, the practitioner observes the heat transfer contained in this
calorimeter lab. This emerges due to the existence of several conserved energy
change events, meaning that the energy contained in electricity is sourced from a
power supply that will flow to the calorimeter and will turn into heat energy. Then,
when stirring upenergy emerges, that is, the mechanical energy that changes into
heat energy is due to the emergence of which is found in the calorimeter and not
created by electrical and mechanical energy, but the result of changes in the shape
of the two energies.
The working principle of a simple calorimeter is known as the mixed method,
namely one sample of the substance is heated to a high temperature measured using
a thermometer, then placed cold water calorimeter. The heat lost in the sample will
be received by water and the calorimeter. By measuring the mixture's final
temperature, type heat can be calculated.
In this experiment also participant use different water masses, different
temperatures so that when the temperature increase is also different, and the voltage
and current issued are also different. A calorimeter is a tool used to determine the
energy that accumulates by measuring temperature changes that occur or changes
in other thermal effects. A calorimeter is a device used for experiments related to
heat. The calorimeter is designed so that heat transfer to the environment occurs to
a minimum. Basically, a calorimeter consists of two vessels separated by an air
space. The inner vessel is made of shiny aluminum to reduce heat absorption by the
vessel wall. The lid of the vessel is made of wood which is a bad conductor so that
not much heat is lost. Calorimeters can be used to measure the heat of a substance.
In the first experiment, the aim was to find the heat energy received by the
calorimeter, in the data that the practitioner got the determination of electrical
energy would be different from the first experiment to the final experiment. The
results we get are in a row 166,2192 cal, 340,704 cal, and 350,784 cal. Because the
practitioner sees the form of the equation of heat energy which is directly
proportional to the mass of water, the heat of type, and changes in time as well, then
the final results that will be obtained will also be different because they are seen
from different temperature changes and different types of water.
In the next experiment calculating electrical energy, where the electrical energy
practicum practiced three experiments, from the data obtained by the practitioner
respectively 855.27 J, 1008 J, and 1008 J. Why in the first experiment of electrical

11. energy in the first experiment different and in the second and third experiments the
same, because in the first experiment when weighing the calorimeter mass the
practitioner used the ohaus balance, and filled the water into the calorimeter using
the ohaus balance, and the temperature was different from the first experiment,
different from the second and third experiments, during the experiment the two
practitioners still use nerca ohaus to weigh the calorimeter mass with the mass of
water in the calorimeter, but when the third experiment the practitioner uses digital
nerca, but why are the results of the second and third experiments the same, and
why the first experiment is not the same initial temperature and temperature change
at the perco first, second and third times, but in the second and third experiments
the initial temperature and final temperature were the same, only the difference
when measuring different calorimeters from the balance sheet in the first, second
and third experiments and the temperature in the first experiment was different, and
the temperature in the second and the three results are the same.
In the last experiment, the practitioner determined the equality in heat, in this
experiment where the results of electrical energy branding inversely with the
amount of heat so that it will get equality contained in heat, from the data obtained
from this practicum are 3.7592, 2, respectively. 1751, 2.1389.
in this calorimeter experiment, thank God, the practitioner can retrieve the data
as expected, and this lab works smoothly under the guidance of Erna.
H. POST PRACTICUM TASKS
1. Explain your analysis of the conservation of energy law in a calorimeter lab?
Answer:
From the understanding of the law of energy conservation itself, energy
cannot be created nor can it be destroyed. The energy conservation law is where
the electrical energy released by the power supply is converted into heat energy
which will be received by the calorimeter. Energy conservation law states that
energy cannot be destroyed and can be created but can only be changed from
one form to another. In nature there is a lot of energy such as electricity, heat
energy, sound energy, but heat energy can only be felt like the heat of the sun.
In everyday life, we often see heating devices that use electrical energy such as
heating jugs, rice cookers, stoves electricity or heating. Basically, these tools
have the same way of working, which is to change the electrical energy flowing
in the wire coil into heat/heat energy. Similarly, the calorimeter is a tool used to

12. measure the amount of heat (calorific value) released. But this time we are
discussing about a simple calorimeter.
2. Compare the energy conversion comparison variables for each experiment?
Answer:
No
.
(V)
Pow
er
sup
ply
mk
(kg)
ma (kg)
T0
(°C)
Tt
(°C)
∆𝑇
(oC
)
Voltage
(V)
I
(A)
t
(s)
1. 6 0.1445 0.08245 27 29 2 5.59
0.8
5
18
0
2. 6 0.1445 0.0845 27 31 4 5.6 1
18
0
3. 6 0.142 0.087 27 31 4 5.6 1
18
0
Of the variables in energy conversion contained on each variable is clearly
different, because seen from the mass of the object, the initial temperature,
changes in temperature, voltage, electric current, the two multimeter devices are
very different from the data obtained from a variable that is water mass, object
mass, initial temperature, final temperature, voltage on the voltmeter, an electric
current to the ammeter. Where in this factor is a factor affecting energy
conversion events?
I. CONCLUSION
Based on the conclusions from this practicum report are:
1. The calorimeter is a tool to measure the heat of the reaction issued.
Calorimeters can be used to calculate the energy in food in the atmosphere
and measure the amount of energy that increases in the calorimeter
temperature.
2. The working principle of the calorimeter is based on the Black Principle
which is stated as follows:
If two objects that have different temperatures are brought close so that
contact occurs, the final temperature of the two objects that have different
temperatures after the thermic balance is reached will be the same.
The amount of heat received = the amount of heat given.

13. 3. The type of heat is the heat needed to increase the temperature of one unit
of mass of the substance by one degree. Heat capacity is the heat needed to
raise the temperature of all objects by one degree. Melting heat is the heat
needed to melt one unit of mass at a fixed temperature.
4. Frozen heat is the heat released when the substance freezes. Normal melting
point is the point where the object changes into a liquid. Steam heat is the
amount of heat needed to evaporate a unit of liquid mass at a fixed
temperature.
5. Dew heat is the amount of heat needed to change form from gas to liquid
one unit of liquid mass at a fixed temperature. The normal boiling point is
the temperature where the pressure of a liquid is the same as the external
pressure experienced by a liquid.
6. The type of calorimeter is divided into two, namely: a simple calorimeter,
and a bomb calorimeter.
7. The value of equality of electric current is influenced by the presence of
large electrical energy and large heat energy.
8. The series is in the amperemeter, and the parallel circuit is on the voltmeter.
9. As a result of the calorimeter wall made of insulating material which serves
to prevent heat propagation to the surrounding environment, thermometer,
and stirrer.
10. Series is used when flowing electricity, and a parallel circuit is used when
connecting a voltage.
J. COMMENTS
1. When conducting a calorimeter practicum, it is hoped that the practitioner
can work together in a fellow team.
2. When the practicum is in progress the practitioner must be careful when
the process of retrieving data on a multimeter.
3. When reading the mass unit value on the balance sheet, both eyes must be
parallel to the Ohaus balance point.
4. When stirring is calibrated along with the power and stopwatch, when the
stopwatch has stopped, it can retrieve data from the lab.
5. Be careful when assembling the calorimeter.

14. K. REFERENCES
Bueche, Frederick. 2006. Schaum's outline of theory and problems of college
physics. Jakarta: Erlangga.
Halliday, Resnick. 2004. Basic Physics. Bandung: ITB.
Purwoko and Fendi. 2007. Physics. Jakarta: Yudhistira.
Sunaryono and Ahmad Taufiq. 2010. Super High School Physics Tips and Tricks.
Jakarta: KAWAHmedia.
Wahyu, et al. 2010. Physical Chemistrya. Jakarta: Rineka Cipta.
Wahyuni, Sri. 2010. Thermodynamic Modules FKIP Jember University. Jember:
University of Jember.
Zemansky, Sears. 1986. Physics for the University. Jakarta: Bina Cipta.
L. ATTACHMENT