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 7.63 g of K2SO4(s) are dissolved in 107.20 g of water, the temperature of the solution drops from 25.27 to 22.68 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.54 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of K2SO4(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. ΔHdissolution =?? 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 7.63 g of K2SO4(s) are dissolved in 107.20 g of water, the temperature of the solution drops from 25.27 to 22.68 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.54 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of K2SO4(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. ΔHdissolution =?? 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
Chapter6: Thermochemistry
Section: Chapter Questions
Problem 112AE: In a bomb calorimeter, the reaction vessel is surrounded by water that must be added for each...
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| 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 7.63 g of K2SO4(s) are dissolved in 107.20 g of water, the temperature of the solution drops from 25.27 to 22.68 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.54 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of K2SO4(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. ΔHdissolution =?? kJ/mol |
Expert Solution
Step 1
Mass of water = 107.20g
Mass of K2SO4 = 7.63
Molar mass of K2SO4 = 174.27 g/mol
Mass of solution = (7.63 + 107.20) g
= 114.83 g
Step 2
Heat released -
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