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 4.53 g of NH4CIO4(s) are dissolved in 111.60 g of water, the temperature of the solution drops from 24.02 to 21.06 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.81 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of NH4CIO4(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AH dissolution 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 4.53 g of NH4CIO4(s) are dissolved in 111.60 g of water, the temperature of the solution drops from 24.02 to 21.06 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.81 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of NH4CIO4(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AH dissolution kJ/mol

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section4.8: Measuring Reaction Enthalpies: Calorimetry

Problem 4.17E

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