In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy 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 97.63grams of nickel to 97.98 °C and then drops it into a cup containing 78.82 grams of water at 23.75 °C. She measures the final temperature to be 32.34 °C. Using the accepted value for the specific heat of nickel (See the References tool), calculate the calorimeter constant.
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy 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 97.63grams of nickel to 97.98 °C and then drops it into a cup containing 78.82 grams of water at 23.75 °C. She measures the final temperature to be 32.34 °C. Using the accepted value for the specific heat of nickel (See the References tool), calculate the calorimeter constant.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter12: Thermodynamic Processes And Thermochemistry
Section: Chapter Questions
Problem 44P
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In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy 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 97.63grams of nickel to 97.98 °C and then drops it into a cup containing 78.82 grams of water at 23.75 °C. She measures the final temperature to be 32.34 °C.
Using the accepted value for the specific heat of nickel (See the References tool), calculate the calorimeter constant.
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