Purpose: This lab taught procedures for determining heat of capacity of a calorimeter and measuring enthalpy of change for three reactions. It also enforced methods of analyzing data obtained through experimentation and calculating enthalpy. These procedures are used in the branch of thermodynamics known as thermochemistry which is the study of energy changes that accompany chemical reactions. Concepts from this lab can be used to determine the potential energy of a chemical reaction. Much of the energy people depend on comes from chemical reactions. For example, energy can be obtained by burning fuel, metabolizing of food or discharging a batter.
Materials and Methods: All work was done with coffee cup …show more content…
Part 1: Determining heat capacity of the calorimeter:
| Mass/g | Temperature | Change in | | | Initial | Final | Temperature | Run 1 | Chilled | 50.963 | 9.6OC | 34.2OC | 24.6OC | | Hot | 50.117 | 54.4OC | 34.2OC | 20.2OC | Run 4 | Chilled | 48.414 | 8.3OC | 30.9OC | 22.6OC | | Hot | 49.918 | 54.0OC | 30.9OC | 23.1OC |
Heat Lost by Heated Water qH=(Cp)(MH)(TH) Run 1 qH=(4.184J/ OC-g)(50.112g)(20.2OC)=4235.31J
Run 4 qH=(4.184J/ OC-g)(49.918g)(23.1OC)=4824.59J
Heat Gained by Chilled Water qC=(Cp)(MC)(TH) Run 1 qC=(4.184J/ OC-g)(50.963g)(24.6OC)=5245.44J