Mass of copper calorimeter: 42.5 ± 0.0001 kg
Specific Heat Capacity of water: 4186 J kg-1 °C-1
Specific Heat Capacity of copper: 390 J kg-1 °C-1
Observation:
Case 1:
Mass of Water: 0.05 ± 0.0001 kg
Initial Temperature of Water and Calorimeter: 22 ± 0.5 °C
Initial Temperature of Metal: 95 ± 0.5 °C
Final Temperature of the mixture: 25 ± 0.5 °C
Case 2:
Mass of Water: 0.08 ± 0.0001 kg
Initial Temperature of Water and Calorimeter: 24 ± 0.5 °C
Initial Temperature of Metal: 95 ± 0.5 °C
Final Temperature of the mixture: 26 ± 0.5 °C
Case 3:
Mass of Water: 0.03 ± 0.0001 kg
Initial Temperature of Water and Calorimeter: 23 ± 0.5 °C
Initial Temperature of Metal: 96 ± 0.5 °C
Final Temperature of the mixture: 27.5 ± 0.5 °C
Data Processing:
Case 1:
Change in temperature of Calorimeter and Water: 25 ± 0.5 - 22 ± 0.5 °C
3 ± 1 °C
Change in temperature of metal: 95 ± 0.5 - 25 ± 0.5 °C
70 ± 1 °C
Heat Lost = Heat Gained
Mass of metal*SIC of metal*change in temperature of metal=(mass of water*SIC of water*change in temperature of water)+(mass of calorimeter*SIC of copper*change in temperature of calorimeter)
0.0246±0.0001 kg * C1 * 70±1 °C = (0.05±0.0001 kg * 4186 J kg-1 °C-1 * 3±1 °C)+(0.0425±0.0001 kg * 390 J kg-1 °C-1 * 3 ± 1 °C)
0.0246 ± 0.0001 * C1 * 70 ± 1 = (0.05 ± 0.0001 * 4186 * 3 ± 1) + (0.0425 ± 0.0001 * 390 * 3 ± 1)
1.722 ± 0.057 * C1 = (627.9 ± 210.5) + (49.725 ± 16.69)
1.722 ± 0.057 * C1 = 677.625 ± 227.19
C1=
C1= 393.5104 ± 144.96 J kg-1 °C-1
Case 2:
Change in temperature of Calorimeter and Water: 26 ± 0.5 - 24 ± 0.5 °C
2 ± 1 °C
Change in temperature of metal: 95 ± 0.5 - 24 ± 0.5 °C
71 ± 1 °C
Heat Lost = Heat Gained
Mass of metal*SIC of metal*change in temperature of metal=(mass of water*SIC of water*change in temperature of water)+(mass of calorimeter*SIC of copper*change in temperature of calorimeter)
0.0246±0.0001 kg * C2 * 71±1 °C = (0.08±0.0001 kg * 4186 J kg-1 °C-1 * 2±1 °C)+(0.0425±0.0001 kg * 390 J kg-1 °C-1 * 2 ± 1 °C)
0.0246 ± 0.0001 * C2 * 71 ± 1 = (0.08 ± 0.0001 * 4186 * 2 ± 1) + (0.0425 ± 0.0001 * 390 * 2 ± 1)
1.747 ± 0.032 * C2 = (669.76 ± 335.72) + (33.15 ± 16.65)
1.747 ± 0.032 * C2 = 702.91 ± 352.37
C2=
C2= 402.3526 ± 209.07 J kg-1 °C-1
Case 3:
Change in temperature of Calorimeter and Water: 27.5 ± 0.5 - 23 ± 0.5 °C
4.5 ± 1 °C
Change in temperature of metal: 96 ± 0.5 – 27.5 ± 0.5 °C
68.5 ± 1 °C
Heat Lost = Heat Gained
Mass of metal*SIC of metal*change in temperature of metal=(mass of water*SIC of water*change in temperature of water)+(mass of calorimeter*SIC of copper*change in temperature of calorimeter)
0.0246±0.0001 kg * C3 * 68.5±1 °C = (0.03±0.0001 kg * 4186 J kg-1 °C-1 * 4.5±1 °C)+(0.0425±0.0001 kg * 390 J kg-1 °C-1 * 4.5 ± 1 °C)
0.0246 ± 0.0001 * C3 * 68.5 ± 1 = (0.03 ± 0.0001 * 4186 * 4.5 ± 1) + (0.0425 ± 0.0001 * 390 * 4.5 ± 1)
1.685 ± 0.031 * C3 = (565.11 ± 127.46) + (74.588 ± 16.75)
1.685 ± 0.031 * C3 = 639.698 ± 144.21
C3=
C3= 379.643 ± 92.57 J kg-1 °C-1
Average heat capacity of a metal =
=
=
Specific Heat Capacity of Metal= 391.8353 ± 100 J kg-1 °C-1
Percentage Uncertainty= Uncertainty/SHC found*100
= 100/391*100
= 25.64%
Conclusion :
From this experiment we can conclude that the specific heat capacity of copper = 391.8353 ± 1oo J approx.
Possible errors:
- Systematic Error in the measurement of variables in instruments such as the thermometer and the weighing scale. The extent is represented by the uncertainty.
- Improper isolation may have led to the system trying to attain equilibrium with the atmosphere and thus reducing the overall final temperature of the system.
- A lot of heat could be lost during the transfer of the solid metal block to the calorimeter
- There could be parallax error while reading the thermometer.
Possible ways of reducing such errors:
- Usage of branded instruments to assure accuracy.
- Using digital thermometers to prevent parallax error and reducing the uncertainty.
- Making the transfer of the metal block quickly so that very less heat energy is escaped.
Candidate Name: - Anurag Saboo