In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat capacity of a solid, or to measure the enthalpy of a solution phase reaction. Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is to use a common metal of known heat capacity. In the laboratory a student heats 91.61 g copper to 98.81 °C and carefully lowers it into a cup containing 76.23 g water at 23.96 °C. She measures the final temperature to be 31.38 °C. Using the accepted value for the specific heat capacity of copper (See the
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat capacity of a solid, or to measure the enthalpy of a solution phase reaction. Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is to use a common metal of known heat capacity. In the laboratory a student heats 91.61 g copper to 98.81 °C and carefully lowers it into a cup containing 76.23 g water at 23.96 °C. She measures the final temperature to be 31.38 °C. Using the accepted value for the specific heat capacity of copper (See the
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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| In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat capacity of a solid, or to measure the enthalpy of a solution phase reaction. Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is to use a common metal of known heat capacity. In the laboratory a student heats 91.61 g copper to 98.81 °C and carefully lowers it into a cup containing 76.23 g water at 23.96 °C. She measures the final temperature to be 31.38 °C. Using the accepted value for the specific heat capacity of copper (See the References tool), calculate the calorimeter constant. |
|
| Calorimeter Constant = J/°C. |
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