LAB Report PHY210 A4AS120211 Group 6 PDF

Preview

Summary

FACULTY OF APPLIED SCIENCESUiTM PERAK (TAPAH CAMPUS)LAB REPORTPHYMECHANICS II AND THERMAL PHYSICSEXPERIMENT TITLE : SPECIFIC HEAT CAPACITYGROUP : A4AS120211(GROUP 6)NAME STUDENT IDNURIN AUNI NAJWA BT MOHD ANAL 2020869122NURUL HAZWANI BINTI MAD SHAH 2020827182SYUKRINA BINTI SULAIMAN 2020609924LECTURE...

Description

FACULTY OF APPLIED SCIENCES UiTM PERAK (TAPAH CAMPUS)

LAB REPORT PHY210 MECHANICS II AND THERMAL PHYSICS EXPERIMENT TITLE GROUP

: SPECIFIC HEAT CAPACITY

: A4AS120211(GROUP 6)

NAME

STUDENT ID

NURIN AUNI NAJWA BT MOHD ANAL

2020869122

NURUL HAZWANI BINTI MAD SHAH

2020827182

SYUKRINA BINTI SULAIMAN

2020609924

LECTURER NAME

: ZUBAINUN MOHAMED ZABIDI

DATE OF SUBMISSION

: 31 MAY 2021

EXPERIMENT 1 METHOD OF MIXTURES: SPECIFIC HEAT CAPACITY THEORY Specific heat capacity of a substance is the amount of heat that must be supplied to increase its temperature by 1˚C for a mass of 1 kg of the substance. Specific heat capacity, c, can be calculated by knowing the amount of heat supplied, Q to a mass, m, of a substance and the resulting increase in temperature, Δθ. When two materials with different temperatures are in contact, heat will flow from higher temperature to the lower temperature, until these two materials reach an equilibrium temperature. The rule of calorimetry principle is also known as 𝐻𝑒𝑎𝑡 𝐿𝑜𝑠𝑠=𝐻𝑒𝑎𝑡 𝑔𝑎𝑖𝑛𝑒𝑑. The quantity of heat absorbed or released by a body is given by (1.1)

𝑄=𝑚𝑐Δ𝜃

In this experiment, a metal of mass, mm that has been heated to a high temperature, θi is dropped into a mass of water, mw at low temperature, θf. When equilibrium is achieved, the new temperature of the water-metal-calorimeter combination is measured as θm. To arrive at this equilibrium temperature, the water and calorimeter must have gained the heat lost by the metals. By neglecting the heat lost to the surrounding, this situation is expressed by equation: 𝑚𝑚 𝑐𝑚 (𝜃𝑖− 𝜃𝑓) = 𝑚𝑤 𝑐𝑤 (𝜃𝑓−𝜃𝑖)

(1.2)

Where:

Theoretical value for metal:

𝑐𝑚 = specific heat capacity of metal

𝑐calorimeter = 𝑐cal = 900 J/kg. ˚C

𝑚𝑚 = mass of metal 𝑚𝑤 = mass of water 𝑐𝑤 =specific heat capacity of water 4200 J/kg. ˚C 𝜃𝑖 =high temperature θf = low temperature

𝑐aluminium = 𝑐al = 900 J/kg. ˚C 𝑐iron = 𝑐fe = 450 J/kg. ˚C 𝑐𝑤ater =𝑐𝑤 =specific heat capacity of water 4200 J/kg. ˚C

Introduction : The objective of this experiment is to measure the specific heat of several different substances such as aluminium block and iron block. This will be done by mixing the two different substances and measuring their initial temperatures and then measuring their final temperature as they come to thermal equilibrium. Objective : -

To measure the specific heat of different substances. To find the total heat loss of the substance when placed in the calorimeter. To measure the amount of heat transferred from the two different metals to water.

Apparatus & materials : 1 unit of Aluminium block, 1 unit of Iron block, 300ml of tap water, 1 unit of calorimeter set, 1 unit of digital thermometer, 1 unit of Hotplate, 1 unit of 500ml graduated cylinder, 1 unit of 350ml beaker, 1 unit of 500ml beaker, 1meter thread, 1 unit of Universal clamp, 1 unit of Retort stand, 1 unit of Digital timer, 1 unit of Electronic balance. Methodology I : 1. 300ml of water was measured by a 500ml graduated cylinder and poured into a 500ml beaker. 2. The water was heated up until the water boiled using a hotplate. 3. The mass of the aluminium block was measured and recorded by using an electronic balance while waiting for the water fully boiled. 4. The aluminium block was tied by a 50cm thread. 5. The aluminium block was hung to a universal clamp that is connected to a retort stand and the aluminium block was heated up in the 500ml beaker of water until the water fully boiled without touching any part of the beaker. 6. The mass of the empty calorimeter with a stirrer was recorded and measured. 7. 200ml of water was measured and poured into the calorimeter. 8. The initial temperature of the calorimeter was measured and recorded for 2 minutes by using a thermometer. 9. The mass of the calorimeter with the water was measured and recorded. 10. The temperature of the aluminium block in the boiling water was measured by using a thermometer and was recorded. 11. Move the aluminium block in the boiling water into the calorimeter quickly. 12. Temperature of the system before it started to fall while stirring the water was measured and recorded. 13. Repeat steps 1-12 by using an iron block. 14. Observations were carried out and the result was measured and recorded.

Methodology II :

Result : Table 2.0: Results for experiment specific heat of capacity

PARAMETER

METAL

AL

FE

Mass of Water inside calorimeter

200 ml

200 ml

Mass Of Metal

0.059 kg

0.06 kg

Mass Of Empty Calorimeter

0.376 kg

0.376 kg

Mass Of Calorimeter with Water

0.570 kg

0.570 kg

Equilibrium Temperature of System

28.7 ˚C

27.2˚C

Initial Temperature of Calorimeter

25.2˚C

25.2˚C

Temperature of Boiling Water

99.4 ˚C

99.3˚C

900 J/kg. ˚C

450 J/kg. ˚C

967.6120 J/kg˚𝐶

533.1484 J/kg ˚𝐶

Specific Heat Capacity Of Metal (Theoretical Value)

Specific Heat Capacity Of Metal (From Calculation)

Analysis of data I : CALCULATION OF THE DATA Discussion : 1) Context : The theoretical value of specific heat capacity for the aluminium block for this experiment is 900J/Kg˚C. However, from the data of the experiment, we got 967.6120 J/kg˚C for the specific heat of the aluminium block. Meanwhile, the theoretical value of specific heat capacity for the iron block is 450 J/kg. ˚C and the specific heat capacity from the data is 533.1484 J/kg. To get more accurate data, a lot of things could be done. First, transfer the aluminium and iron block as fast as possible so less heat will be absorbed or released to the environment. Thermometer used can be changed to a digital thermometer as it is more accurate. 2) Experimental error : ● Heat can escape through the calorimeter as well as through the thermometer.There could also be parallax error when reading the temperature off the thermometer.Taking longer time to transfer metal to water will result in heat loss and a less accurate result. ● The prevention are to close the calorimeter tightly so that less heat escapes to the environment. To prevent parallax error, use a digital thermometer as it gives reading to a more accurate degrees.Try to transfer the metal faster to prevent too much heat loss so more accurate data could be taken.

3) Question : a. Calculate the specific heat capacity of Al and Fe metal blocks. (refer appendix for theoretical value, Ccal and Cw). Specific heat capacity,c of Aluminium: 𝑀 𝐶 (𝜭 − 𝜭 ) = [𝑀𝑤 𝐶𝑤 + 𝑀 𝑚

𝑎𝑙

𝑖

𝑓

𝑐𝑎𝑙

𝐶 ][𝜭 − 𝜭 ] 𝑖

𝑓

𝑐𝑎𝑙

[𝑀𝑤 𝐶𝑤+𝑀

𝑐𝑎𝑙

𝐶𝑎𝑙 =

𝐶 ][𝜭 −𝜭 ] 𝑖

𝑓

𝑐𝑎𝑙

𝑀 (𝜭 −𝜭 ) 𝑎𝑙

𝑖

𝑓

=

(0.376×900)+(0.194×4200)(28.7−25.2) [0.059(99.4−28.7)

=

(1153.2×3.5) (0.059×70.4)

=

4036.2 4.1713

= 967. 6120 𝐽/𝐾𝑔℃

Specific heat capacity,c of Ferum : 𝑀 𝐶 (𝜭 − 𝜭 ) = [𝑀𝑤 𝐶𝑤 + 𝑀 𝑓𝑒

𝑓𝑒

𝑖

𝑓

𝐶 ][𝜭 − 𝜭 ]

𝑐𝑎𝑙

𝑖

𝑓

𝑐𝑎𝑙

[𝑀𝑤 𝐶𝑤+𝑀

𝐶 ][𝜭 −𝜭 ]

𝑐𝑎𝑙

𝑖

𝑓

𝑐𝑎𝑙

𝐶𝑓𝑒 =

𝑀 (𝜭 −𝜭 ) 𝑓𝑒

𝑖

𝑓

=

(0.376×900)+(0.194×4200)(27.2−25.2) 0.06(99.3−27.2)

=

(1153.2×2) (0.06×72.1)

=

2306.9 4.326

= 533. 1418 𝐽/𝐾𝑔℃ b. Calculate the percentage difference between your calculated specific heat capacity and its theoretical value. (refer appendix) Specific heat capacity of aluminium, Al Theoretical value = 900𝐽/𝐾𝑔℃ Experimental value= 967.612𝐽/𝐾𝑔℃

=

967.612−900 900

× 100

= 7. 512% Specific heat capacity of ferum, Fe Theoretical value= 450𝐽/𝐾𝑔℃ Experimental value= 533.1484𝐽/𝐾𝑔℃

=

533.1484−450 900

× 100

= 18. 48%

c. Why should you stir the water at the end of the experiment before the temperature reading is taken? To prevent hot-spots, it is important to continuously stir the water because temperature is a measure of the kinetic energy of the particles in the water and stirring provides kinetic energy of water in the calorimeter scattered. Stirring is needed to make sure the rising temperature of water is uniform in calorimeter experiment.

d. Why is water used in the experiment as a cooling system? Water has a very high Specific Heat Capacity. A lot of energy needs to be absorbed by water to increase its temperature. Hence, the temperature of the system decreases much more than the temperature of the water increases. This is why water is a very effective cooling agent in this experiment. Conclusion : By using the method of mixture technique, the specific heat capacity of Aluminium block was found to be 967.6120 J/kg ˚𝐶 and having 7.512% error from the theoretical value of 900 J/kg. ˚C. As for Iron, the specific heat capacity was 533.1484 J/kg˚𝐶 with its percentage error of 18.48% from its theoretical value of 450 J/kg˚𝐶 Hence, the objective of the experiment was not acceptable. As we can conclude that the calorimeter was not completely isolated and heat was lost also before the hot water was poured into the calorimeter and the room temperature is the one affecting the values of our results. Meanwhile, in the experiment determining the specific heat of aluminium and iron blocks, we got higher percentage errors; these are due to heat loss to the surroundings while we are trying to transfer the hot aluminium and iron blocks from the beaker to the calorimeter, boiling point of those metals are too long, room temperature, and apparatuses. However we can conclude that the specific heat of metals is lower than the specific heat of water.

References : Ahmed Musawar, (2018), Principles of Physics https://www.studocu.com/en-us/document/queensborough-community-college/principles-of-p hysics/coursework/lab-10-ph-101-lab-report/2150046/view Phy022groupone, (2014), Experiment 6 – Heat and Calorimetry, https://phy022groupone.wordpress.com/2014/12/10/experiment-6-heat-and-calorimetry/ Unknown,(None) Experiment Specific Heat Capacity https://www.austincc.edu/physci_tf/Physics/labs/riogrande/phys1401/SpecificHeat Unknown, (2017), Specific Heat Capacity Report https://www.studocu.com/en-gb/document/sheffield-hallam-university/engineering-practice-el ectrical-and-electronic/essays/specific-heat-capacity-report/1575019/view...