MAPUA INSTITUTE OF TECHNOLOGY Department of Physics E302: HEAT AND CALORIMETRY GICALE, PATRICK EMMANUEL T.
[email protected]/2014106318/CE-2 PHY12L-B2 Group 2
SCORE Signed Data Sheet (5)
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Observations Observation s & Results (15)
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Graphs (10)
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Conclusion (15)
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References (5)
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Photos (10)
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Performance (40)
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TOTAL (100)
17 May, 2016
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E302: HEAT AND CALORIMETRY Gicale, Patrick Emmanuel T.1, 1 School of Civil, Environmental, and Geological Engineering , Mapúa Institute of Technology 658 Muralla St., Intramuros, Manila City, Philippines
[email protected]
OBSERVATIONS AND RESULTS
Materials possess, it may be a solid, liquid or a gas, a specific amount of heat, which differs from all of the bodies also relative to its size, needed to be absorb to raise its temperature and this is Specific Heat. In our experiment, we are tasked to determine the metal samples’, aluminium and copper, specific heat capacity through the formula of sensible heat. (1) The second part of the experiment is the determination of the latent heat of fusion of ice. It is a constant which will dictates the needed heat to be absorb or taken off. Latent Heat of fusion is solve through the formula. (2) After doing two trials of determining the specific heat capacity of the two metals, we achieved a relevant specific heat capacity. Below are the relevant values that we’ve gathered.
= ∆ =
Table 1: Data Gathered for Determining the Specific Heat of Metals Aluminium metal Copper metal Mass of metal (g) 32.7 19.6 Mass of calorimeter (g) 46.3 46.3 Mass of water (g) 127.1 133.3 o Initial temperature of metal ( C) 100 100 o Initial temperature of calorimeter ( C) 26 27 o Initial temperature of water ( C) 26 27 o Final temperature of mixture ( C) 30 28 Experimental specific heat of metal 0.2397 0.1016 o (cal/g-C ) Actual specific heat of metal (cal/g0.2174 0.0932 o C) Percentage of error 10.26% 9.0035%
As you can see, the following metals have different specific heat where aluminium being the greater. Hence, the aluminium metal needed greater heat than the copper to raise its temperature. Below were represents the data gathered to determine the ice’s latent heat of fusion and as you can see, the experimental values have a minimal deficiency to its actual value. Sources of error will be discussed on the conclusion.
Table 2: Data Gathered to Determine the Latent Heat of Fusion of Ice 1st Trial 2nd Trial Mass of calorimeter (g) 46.3 46.3 Mass of water (g) 114.3 139.2 Mass of mixture (g) 160.3 167.6 Mass of ice (g) 46.3 46.3 o Initial temperature of ice ( C) 0 0 o Initial temperature of calorimeter ( C) 62 65 o Initial temperature of water ( C) 62 65 o Final temperature of mixture ( C) 19 34 Experimental latent heat of fusion 96.5015 65.9403 (cal/g) Actual specific latent heat of fusion 80 80 (cal/g) Percentage of error 17.57 % 20.63 %
∆ + ∆ + ∆ = 0 (46.(1327.) 0.1)2174(30−26 (30−26)) + + (46.3)0.0932 (28−27) + ( ) 1 33. 3 (2 8−27) + (32.7)(30−100) = 0 (19.6)(28−100) = 0 = . − () % % 0. 0 932 − 0. 1 016 / = | | 100 0.= | 2174 0.2174 − 0.2397 / 0. 0 932 / / |100 % = . % % = . % ( ) ( ) ( ) − + − + + − 0 = 0 (114.3) (19−62)( +46.(436.)3(1)9−0) (0.2174 =0)(19−62) + (46.3) +
Below is a sample computation for solving the specific heat.
Aluminium metal:
Copper metal:
o c =0.2397 cal/g-C m
o c =0.1016 cal/ g-C m
Sample Computation for solving Latent Heat of Fusion of ice:
L F =96.5015
GRAPHS
The table below represents the comparison of the relevant values that we’v e gathered to the actual value. As you can see, Aluminum metal has greater specific heat capacity thus, the metal needs greater heat to raise its temperature.
Y T I C A P A C T 0.3 A E 0.2 H C I 0.1 F I C 0 E P S
Specific Heat Capacity of the Metals 0.2397 0.2174 1.02E-01 0.0932
Experimental Value of Specific Heat Capacity
Actual Value of Specific Heat Capacity COMPARISON OF RELEVANT VALUE TO THE ACTUAL VALUE Aluminium Metal
Copper Metal
The table below represents the difference of th e experimental value from the actual value. As you can see, the following experimental data are close to the actual value. F O T A N E O150 H I S T U100 N F E 50 T A L 0
Latent Heat of Fusion (Ice) 80
Actual Value
9.65E+01
Trial 1
6.59E+01
Trial 2
VALUE PER TRIAL
CONCLUSIONS
Objectively, we've solved the metals’ specific heat and the ice’s latent heat of fusion. Comparing the experimental data to the actual values, the percentage error from the first part are 10.26% (Aluminum) and 9.0035% (Copper). Hence, the data gathered is acceptable. Next part, the comparison from the experimental values to the actual values are somehow big. The percentage error is 20.63% and 17.57%. Possible source of these big errors might be the initial temperature of the water. Since, the environment is cold and heat travels from hot to cold thus, we can say that the ice didn't melt. Thus, the final temperature of the mixture might not be accurate. To improve the data, the experiment must be done in a normal room temperature. Based on the data, specific heat capacity is relative to its mass and the heat transferred. As to the data, since the change of the temperature of calorimeter and water of the aluminium is greater than the copper hence the heat transferred is greater than the mass. Thus, aluminium’s specific heat is still greater. As to the latent heat of fusion, it is also relative to the heat transferred and mass. Since the mass of the ice of both trial is the same, the greater the heat transferred the greater the computed latent heat of fusion. Thus, we can say that it is proportional to the heat transferred and inversely proportional to the mass. Whilst, the specific heat is also proportional to the heat transferred but inversely proportional to mass and the temperature change. REFERENCES Serway, R. A., & Jewett Jr., John W. (2014). University Physics. Philippines: Cengage Learning Asia Pte Ltd.
PHOTOS
Photo 1: Measuring the temperature of the calorimeter.
Photo 2: Measuring the mass of calorimeter.
Photo 3: Boiling the copper metal.
Figure 4: Set-up of the experiment
