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. A chunk of gold weighing 19.44 grams and originally at 97.29 °C is dropped into an insulated cup containing 76.16 grams of water at 21.34 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.54 J/°C. Using the accepted value for the specific heat of gold (See the References tool), calculate the final temperature of the water. Assume that no heat is lost to the surroundings.
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. A chunk of gold weighing 19.44 grams and originally at 97.29 °C is dropped into an insulated cup containing 76.16 grams of water at 21.34 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.54 J/°C. Using the accepted value for the specific heat of gold (See the References tool), calculate the final temperature of the water. Assume that no heat is lost to the surroundings.
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
Chapter6: Thermochemistry
Section: Chapter Questions
Problem 112AE: In a bomb calorimeter, the reaction vessel is surrounded by water that must be added for each...
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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.
A chunk of gold weighing 19.44 grams and originally at 97.29 °C is dropped into an insulated cup containing 76.16 grams of water at 21.34 °C.
The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.54 J/°C.
Using the accepted value for the specific heat of gold (See the References tool), calculate the final temperature of the water. Assume that no heat is lost to the surroundings.
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