Calorimetry Lab

Eric Bryan
Period 4

Calorimetry Lab

Theory: To most people heat and temperature are generally the same thing. But really in a scientific sense there is still a similarity between them but they are different concepts. Temperature is the measure of the average energy of molecular motion in a substance. Heat is the total energy of molecular motion in a substance. Temperature is not energy like heat is, it is just measure of it. Now there is also a difference between heat and thermal energy. Heat is an energy that is transferred between different substances due to a temperature gradient between them while thermal energy is just the energy of a substance related to its temperature. One more thing is specific heat is the amount of heat per unit mass required to raise the temperature by one degree Celsius. For example the specific heat of water is
4186 joule/gramoC. This is higher than any other common substance, which means it has a very large role in temperature regulation. It takes a lot to chance its temperature. Calorimetry is the measure of heat in chemical reactions. How this is done is a substance is put in water and then the temperature change of the water is measured to mind how much the particular substance was able to change it.

DATA:

PART A:

Mass/Volume/Density of Metals Steel Copper Aluminum
Mass (g) ±.1 75.1 56.6 34.7
Volume (ml) ±1 10 7 13
Density (g/ml) 7.5 ±.08 7.3 ±.08 2.7 ±.08

Specific Heat of Metals Steel Copper Aluminum
Hot Plate Temp. (oC) ±.1 93.6 93.5 93.5
Room Temp (oC) ±.1 22.4 22.3 22.3
Combined Temp. (oC) ±.1 25.9 24.0 24.5
Specific Heat (J/kg0C) 504.3 324.0 671.1

PART B:

Specific Heat of Water 700C 800C 900C
Room Temp (oC) ±.1 21.2 24.7 24.9
Hot Plate Temp. (oC) ±.1 70 80 90
Final Temp. (oC) ±.1 41.5 47.2 51.0
Temp. Final (oC) 45.6 52.4 57.5

Part C:

Heat Fusion of Ice Ice Mass (g) ±.1 63.9 46.0 43.5
Initial Temp (oC) ±.1 21.8 20.4 23.5
Final Temp (oC) ±.1 4.8 6.6 6.0