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 3.95 g of CuCl2(s) are dissolved in 108.60 g of water, the temperature of the solution increases from 23.05 to 26.27 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.86 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CuCl2(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 3.95 g of CuCl2(s) are dissolved in 108.60 g of water, the temperature of the solution increases from 23.05 to 26.27 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.86 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CuCl2(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AHdissolution kJ/mol
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section: Chapter Questions
Problem 96IL: Insoluble PbBr2(s) precipitates when solutions of Pb(NO3)2(aq) and NaBr(aq) are mixed. Pb(NO3)2(aq)...
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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 3.95 g of CuCl2(s) are dissolved in 108.60 g of
water, the temperature of the solution increases from 23.05 to 26.27 °C.
The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a
separate experiment to be 1.86 J/°C.
Based on the student's observation, calculate the enthalpy of dissolution of CuCl,(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%2F397ac19d-419d-47a7-b806-aa011335da74%2Ff519b202-b97a-4500-9732-fe99baa58516%2Fvxhldce_processed.png&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 3.95 g of CuCl2(s) are dissolved in 108.60 g of
water, the temperature of the solution increases from 23.05 to 26.27 °C.
The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a
separate experiment to be 1.86 J/°C.
Based on the student's observation, calculate the enthalpy of dissolution of CuCl,(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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