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 3.23 g of CuCl2(s) are dissolved in 100.30 g of water, the temperature of the solution increases from 25.75 to 28.61 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.83 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 3.23 g of CuCl2(s) are dissolved in 100.30 g of water, the temperature of the solution increases from 25.75 to 28.61 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.83 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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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