Lab Report Name: ____________________
Section: ___________________
EXPERIMENT: Specific Heat Capacity of Metals
DATA TABLE 1:
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Object Description – |
First Metal |
Second Metal |
|
Room temperature, oC |
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|
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Mass of water in calorimeter, 25 ml = 25 g |
|
|
|
Mass of first metal object |
|
|
|
Starting temperature of water (room temp) |
|
|
|
Starting temperature of object (room temp) |
|
|
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Highest final temperature of water & object |
|
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DATA TABLE 2 – Part 1:
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Objects |
Mass (g) |
T initial |
T final |
DT |
C (cal/g oC) |
|
Water in calorimeter |
|
|
|
|
|
|
First metal |
|
|
|
|
|
Percent error of your experimentally derived value: _____________
DATA TABLE 2 – Part 2:
|
Objects |
Mass (g) |
T initial |
T final |
DT |
C (cal/g oC) |
|
Water in calorimeter |
|
|
|
|
|
|
Second metal |
|
|
|
|
|
Percent error of your experimentally derived value: _____________
Questions:
A. Why is it a good idea to start with room temperature water in the calorimeter?
B. Why did we ignore the calorimeter in our calculation, although it is listed in the original equation?
C. When eating apple pie, you may have noticed that the filling seems to be much hotter than the crust. Why is this? What can you conclude about the specific heat of the fillings vs. the specific heat of the crust?
D. Is the heat exchange between the metal and the water in the calorimeter by radiation, conduction or convection? Why?
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