In the laboratory a general chemistry student finds that when 0.73 g of KOH(s) are dissolved in 100.40 g of water, the temperature of the solution increases from 22.85 to 24.69 °C. Based on the student's observation, calculate the enthalpy of dissolution of KOH(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water, which is 4.184J/g*C.

In the laboratory a general chemistry student finds that when 0.73 g of KOH(s) are dissolved in 100.40 g of water, the temperature of the solution increases from 22.85 to 24.69 °C. Based on the student's observation, calculate the enthalpy of dissolution of KOH(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water, which is 4.184J/g*C.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 85AP

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