| Physical Science - FME [Phys 101] Spring 2004 |
[1] Get into the groups that you used on Monday. The second column of the table below lists the amount of water that your group will be using. Use a graduated cylinder to pour this amount of water into your styrofoam cup.
Group
|
Cylinder Composition
|
Volume of Water (mls)
|
Car Bombs
|
Aluminum
|
50
|
Group A
|
Aluminum
|
80
|
Pink Flamingos
|
Aluminum
|
100
|
Team Choir
|
Brass
|
50
|
Dynamites
|
Brass
|
80
|
JRKC
|
Brass
|
100
|
[2] Use a thermometer to measure the temperature of the water in your cup. Record this temperature.
[3] Head up to the front of the room and ask John for either an Aluminum or Brass cylinder, as indicated in the above table. As soon as this cylinder is placed into your styrofoam cup, begin to monitor the temperature carefully. Record the highest temperature that your water reaches.
[4] Determine the change in temperature of your water. Realizing that it takes 1 calorie to raise the temperature of 1 ml of your water by 1° C, determine the number of calories of heat that must have flowed into your water from the cylinder.
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[5] Calculate the temperature change of your cylinder. By looking at the temperature change, determine the number of calories that flowed out of it for EACH DEGREE by which it changed temperature. |
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[6] The mass of the Aluminum cylinders is 17 grams, while the mass of the Brass cylinders is 54 grams. Using this information, determine the number of calories that flowed out of EACH GRAM of the cylinder for each degree by which it changed temperature. When you have done this, you have answered the question "How many calories are required to change the temperature of 1 gram of this substance (aluminum or brass) by one degree Celsius?". The answer for water was "1". Is it the same for these metals? |