A student determines the heat of dissolution of solid cesium sulfate using a coffee-cup calorimeter of negligible heat capacity. When 16.2 g of Cs₂SO4(s) is dissolved in 101.00 g of water, the temperature of the solution drops from 25.00 to 23.12 °C. Based on the student's observation, calculate the enthalpy of dissolution of Cs₂SO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. AH dissolution kJ/mol

A student determines the heat of dissolution of solid cesium sulfate using a coffee-cup calorimeter of negligible heat capacity. When 16.2 g of Cs₂SO4(s) is dissolved in 101.00 g of water, the temperature of the solution drops from 25.00 to 23.12 °C. Based on the student's observation, calculate the enthalpy of dissolution of Cs₂SO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. AH dissolution 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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A student determines the heat of dissolution of solid cesium sulfate using a coffee-cup
calorimeter of negligible heat capacity.
When 16.2 g of Cs₂SO4(s) is dissolved in 101.00 g of water, the temperature of the solution drops
from 25.00 to 23.12 °C. Based on the student's observation, calculate the enthalpy of dissolution
of Cs₂SO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.
AH dissolution=
kJ/mol
ant P Calorimetry - Heat of Solution (Calorimete...: This is group attempt 1 of 10
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