A student determines the heat of dissolution of solid cesium perchlorate using a coffee-cup calorimeter of negligible heat capacity.When 3.45 g of CsClO4(s) is dissolved in 117.00 g of water, the temperature of the solution drops from 25.00 to 23.25 °C. Based on the student's observation, calculate the enthalpy of dissolution of CsClO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.
A student determines the heat of dissolution of solid cesium perchlorate using a coffee-cup calorimeter of negligible heat capacity.When 3.45 g of CsClO4(s) is dissolved in 117.00 g of water, the temperature of the solution drops from 25.00 to 23.25 °C. Based on the student's observation, calculate the enthalpy of dissolution of CsClO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.
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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A student determines the heat of dissolution of solid cesium perchlorate using a coffee-cup calorimeter of negligible heat capacity.
When 3.45 g of CsClO4(s) is dissolved in 117.00 g of water, the temperature of the solution drops from 25.00 to 23.25 °C. Based on the student's observation, calculate the enthalpy of dissolution of CsClO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.
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