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 10.10 g of CsBr(s) are dissolved in 116.70 g of water, the temperature of the solution drops from 23.45 to 20.60 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.55 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CsBr(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water.
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 10.10 g of CsBr(s) are dissolved in 116.70 g of water, the temperature of the solution drops from 23.45 to 20.60 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.55 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CsBr(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water.
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 10.10 g of CsBr(s) are dissolved in 116.70 g of water, the temperature of the solution drops from 23.45 to 20.60 °C.
The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.55 J/°C.
Based on the student's observation, calculate the enthalpy of dissolution of CsBr(s) in kJ/mol.
Assume the specific heat of the solution is equal to the specific heat of water.
ΔHdissolution = kJ/mol
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