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CHEMICAL ENGINEERING LABORATORY 1
(BKC1752)
Title of Experiment : Specific Heat
Date of Experiment : 17/04/2023
Instructor’s Name : Dr. Siti Hatijah Binti Mortan
Group No. : 01
Section : 02G
List of Students:
Name ID
1. KIVENRAJ A/L BALAN KA22049
2. PRIVEEN RAJ THEVAR A/L SELVAN KA22081
3. HARITH SUFYAN BIN SYAMSUL AZRI KA22074
4. NARMATHA A/P RAJALINGGAM KA22105
5. SHARUL SAZWAN BIN MOHD. AHMADI KA22066
6. EMMANUEL PAUL A/L RICHARD PAUL KA22087
Marks:
1
Tear here
Subject Code: BKC1752
Title of Experiment: Date Submitted :
1. Abstract 6. Results
2. Methodology flowchart 7. Discussion
3. Data Tabulation 8. Conclusions
4. Graph 9. References
5. Calculations 10. Grammar and Spelling
TOTAL
Received by;
( )
Submitted by;
( )
ABSTRACT
The title of this experiment is called Specific Heat. Specific heat can be defined as the
amount of energy to raise the temperature of 1 gram of a substance by 1°C. In SI units,
specific heat capacity, c is the amount of heat in joules required to raise 1 gram of a substance
1 Kelvin. It minstanceressed as J/kg·K For an instance, the specific heat capacity of water is
4184 J/kg·°C. So, this means that it takes 4184 Joules of energy to raise 1 gram of water by
1°C. The objectives of this experiment are to determine the specific heat of a metal. In this
experiment, the metal used is copper. Besides, this experiment is carried out to determine the
quantity and direction of heat flow for the dissolution of a salt. In this experiment, the salt
used is sodium thiosulphate. The study of specific heat falls under the category of
Thermochemistry which is further divided into the category of Calorimetry. An instrument
which is known as calorimeter is used to measure specific heat. 10g of copper metal is
measured and transferred in a test tube that was placed in a beaker that contains water, which
its level exceeds the level of copper metal sample. The beaker is then boiled. The test tube
containing copper metal is then taken out of the boiling water and placed in a calorimeter
which contains 20ml of room temperature water. The heat that was absorbed by the copper
metal is measured by the temperature change the metal causes in the room temperature water.
This exact same method is repeated by using 5g of sodium thiosulphate salt. For the
procedures that were executed with copper metal, the value of the specific heat capacity of
water that has been calculated is 0.3782 J/g°C. The theoretical value for the specific heat
capacity is 0.385 J/g°C. Meanwhile, the percentage error of specific heat capacity is
0.0177%. For the procedures that were executed with sodium thiosulphate salt, the enthalpy
of solution is +7903.3892 J/ mol.
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METHODOLOGY
Table 1: Method for Specific Heat of a Metal (Part A)
Table 2: Method for Enthalpy (Heat) of Solution for the Dissolution of a Salt (Part B)
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RESULTS
Part A: Specific Heat of a Metal
Temperature of water in equilibrium = 26°C
Temperature of metal in equilibrium = 26°C
Mass of calorimeter = 2.7635g
Mass of water = 20.1863g
Mass of calorimeter + water = 22.9498g
Mass of lid = 9.4977g
Temperature of 60 seconds intervals in 5 minutes for water in calorimeter to achieve thermal
equilibrium:
Temperature of 30 seconds intervals of 3 minutes for water when metal is mixed:
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Intervals Temperature
60 26
120 26
180 26
240 26
300 26
Interval
s Temperature
30 27
60 27.9
90 28.5
120 28.8
150 29
180 29
Diagram 4.1: Graph of Temperature versus Time
Part B: Enthalpy of Solution for the Dissolution of a Salt
Temperature of water in equilibrium = 26°C
Temperature of metal in equilibrium = 26°C
Mass of dry calorimeter = 2.3414g
Mass of water = 19.8970g
Mass of calorimeter + water = 22.2384g
Mass of lid = 9.8817g
Temperature of 15 seconds intervals in 60 seconds for water in calorimeter to achieve thermal
equilibrium:
5
Intervals Temperature
15 26
30 26
45 26
60 26
0 30 60 90 120 150 180 210
26
26.5
27
27.5
28
28.5
29
29.5
Graph of Temperature(◦c) versus Time (s)
Time
Temperature
Temperature of 30 seconds intervals of 3 minutes for water when metal is mixed:
Diagram 4.2: Graph of Temperature versus Time
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Intervals Temperature
15 23
30 22.5
45 22
60 22
75 21.5
90 21
105 20.8
120 20.4
135 20.1
150 20
165 20
180 20
0 15 30 45 60 75 90 105 120 135 150 165 180 195
18.5
19
19.5
20
20.5
21
21.5
22
22.5
23
23.5
Graph of Temperature(◦c) versus Time (s)
Time
Temperature
DISCUSSION
QUESTION 1
Calculation of the specific heat of copper
-The temperature change for the copper, ()
= Final temperature of the copper – Initial temperature of the copper
= 29°C - 96°C
= -67°C
negative temperature change indicates that heat was lost.
-The temperature change or the water, ()
= Final temperature of the water – Initial temperature of the water
= 29°C - 26°C
= 3°C
positive temperature change indicates that heat was absorbed.
-Heat absorbed by the water, (
= mcΔT
= x x
= 20.1863g x 4.184 J/g°C x 3°C
= 253.3784 J
Specific heat capacity of copper,
At thermal equilibrium the amount of heat loss by the copper equals to the amount of
heat gained by the water
Heat loss by the copper = Heat gained by the water
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= 253.3784 J
-253.3784 J = 10.000 g x x (-67°C)
= 0.3782 J/g°C
Calculation of percentage of error for specific heat capacity of copper,
Given the theoretical value for the specific heat capacity is 0.385 J/g°C
(theengineeringmindset.com)
=
= 0.0177
QUESTION 2
Calculation for Enthalpy of Solution for ��2�2�3,
-The temperature change for the water, ()
= Final temperature of the water – Initial temperature of the water
= 20°C - 23°C
= -3°C
Heat loss by the water, (
= mcΔT
= x x
= 19.8970g x 4.184 J/g°C x -3°C
= -249.7471 J
Number of mol of ��2�2�3
8
-
=
= 0.0316 mol
Enthalpy of Solution for ��2�2�3,
At thermal equilibrium the amount of heat loss by the water equals to the amount of heat
gained by 𝑁 𝑁 2𝑁2𝑁3
Heat gained by the ��2�2�3 = Heat loss by the water
=
= 7903.3892 J/mol
= +7903.3892 J/mol
Based on the calculation above, the enthalpy of solution for 𝑁𝑁2𝑁2𝑁3, ∆𝑁 is +7903.3892
J/mol. The sign of the enthalpy change indicates the direction of heat flow during a chemical
reaction or physical process. When the enthalpy change is positive, it means that the system
has absorbed energy from the surroundings, which results in an increase in the internal energy
of the system. This means that the system becomes colder, and the surroundings become
hotter, as heat flows from the surroundings into the system. Therefore, a positive value of
enthalpy indicates that heat is flowing into the system. This relationship between enthalpy
and heat flow is known as the first law of thermodynamics, which states that energy cannot
be created or destroyed, only transferred, or converted from one form to another.
CONCLUSION/ RECOMMENDATION
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By the end of this experiment, the objective of this experiment, which is to determine
the specific heat of a metal, has been achieved. In this experiment, the metal used is copper.
The temperature of thermal equilibrium of water and copper is 26 °C achieved by 60 seconds
intervals in 5 minutes. Temperature of 30 seconds intervals of 3 minutes for water when
metal is mixed recorded to get the temperature change of copper. The temperature change of
water is 3°C. The positive temperature change indicates that heat was absorbed. Heat
absorbed by water is 253.3784 J. At thermal equilibrium the amount of heat loss by the
copper equals the amount of heat gained by the water. Hence, the value of specific heat
capacity of water that has been calculated is 0.3782 J/g°C. The theoretical value for the
specific heat capacity is 0.385 J/g °C. The percentage error of specific heat capacity is
0.0177%. Besides, this experiment is carried out to determine the quantity and direction of
heat flow for the dissolution of a salt. The heat that was absorbed by the copper metal is
measured by the temperature change the metal causes in the room temperature water. This
exact same method is repeated by using 5g of sodium thiosulphate salt. At thermal
equilibrium the amount of heat loss by the water equals to the amount of heat gained by
𝑁𝑁2𝑁2𝑁3. The enthalpy of solution for 𝑁𝑁2𝑁2𝑁3, ∆𝑁 is +7903.3892 J/mol. The sign of
enthalpy change is positive; thus, the system has absorbed energy from the surroundings.
As recommendation to improve and get precise values for the experiments results, is
using digital calorimeter instead of calorimeters that are made of Styrofoam. Digital
calorimeters are electronic devices that use a thermistor or thermocouple to measure
temperature changes in a reaction. They are generally more precise and accurate than
calorimeters made of Styrofoam because they can measure very small changes in
temperature. Digital calorimeters can also automatically calculate the heat of the reaction
based on the temperature changes, which can save time and reduce errors in calculations.
However, digital calorimeters can be expensive and require a power source, which makes
them less portable than calorimeters made of Styrofoam. On the other hand, calorimeters
made of Styrofoam, are generally less precise and accurate than digital calorimeters and more
susceptible to heat loss and can be affected by external factors such as air currents.
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REFERENCE
1. Evans, P. (2016), Specific heat capacity of materials. Specific heat capacity of
materials - The Engineering Mindset
2. Encyclopedia Britannica. (n.d.). Understanding enthalpy, exothermic, and
endothermic reactions. Understanding enthalpy, exothermic, and endothermic
reactions | Britannica
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APPENDIX
Figure 1; Measurement mass of calorimeter.
Figure 2; Boil the water and put the test tube containing metal in the beaker.
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