A student determines the heat of dissolution of solid ammonium chloride using a coffee-cup calorimeter of negligible heat capacity. When 2.84 g of NH4Cl(s) is dissolved in 109.00 g of water, the temperature of the solution drops from 25.00 to 23.20 °C. Based on the student's observation, calculate the enthalpy of dissolution of NH4Cl(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. ΔHdissolution = kJ/mol
A student determines the heat of dissolution of solid ammonium chloride using a coffee-cup calorimeter of negligible heat capacity. When 2.84 g of NH4Cl(s) is dissolved in 109.00 g of water, the temperature of the solution drops from 25.00 to 23.20 °C. Based on the student's observation, calculate the enthalpy of dissolution of NH4Cl(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. 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
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 ammonium chloride using a coffee-cup calorimeter of negligible heat capacity.
When 2.84 g of NH4Cl(s) is dissolved in 109.00 g of water, the temperature of the solution drops from 25.00 to 23.20 °C. Based on the student's observation, calculate the enthalpy of dissolution of NH4Cl(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.
ΔHdissolution = kJ/mol
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