When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 17.71 g of BaCl2(s) are dissolved in 101.40 g of water, the temperature of the solution increases from 23.57 to 26.58 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.76 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of BaCl2(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AHdissolution kJ/mol
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 17.71 g of BaCl2(s) are dissolved in 101.40 g of water, the temperature of the solution increases from 23.57 to 26.58 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.76 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of BaCl2(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AHdissolution kJ/mol
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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![When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can
be determined using a coffee cup calorimeter.
In the laboratory a general chemistry student finds that when 17.71 g of BaCl2(s) are dissolved in 101.40 g
of water, the temperature of the solution increases from 23.57 to 26.58 °C.
The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a
separate experiment to be 1.76 J/°C.
Based on the student's observation, calculate the enthalpy of dissolution of BaCl2(s) in kJ/mol.
Assume the specific heat of the solution is equal to the specific heat of water.
AHdissolution
kJ/mol](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdcf7bbff-0080-454e-ba58-fca63022c2bd%2F5c5b2c50-c6da-4415-82d0-0c2722370cb2%2Fro3xeah_processed.jpeg&w=3840&q=75)
Transcribed Image Text:When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can
be determined using a coffee cup calorimeter.
In the laboratory a general chemistry student finds that when 17.71 g of BaCl2(s) are dissolved in 101.40 g
of water, the temperature of the solution increases from 23.57 to 26.58 °C.
The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a
separate experiment to be 1.76 J/°C.
Based on the student's observation, calculate the enthalpy of dissolution of BaCl2(s) in kJ/mol.
Assume the specific heat of the solution is equal to the specific heat of water.
AHdissolution
kJ/mol
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