0.700 moles of an unknown solid is placed into water to make 150.0 mL of solution. The solution's temperature decreases by 7.61°C. Calculate ∆H, in kJ/mol, for the dissolution of the unknown solid. (The specific heat of the solution is 4.184 J/g・°C and the density of the solution is 1.02 g/mL).
0.700 moles of an unknown solid is placed into water to make 150.0 mL of solution. The solution's temperature decreases by 7.61°C. Calculate ∆H, in kJ/mol, for the dissolution of the unknown solid. (The specific heat of the solution is 4.184 J/g・°C and the density of the solution is 1.02 g/mL).
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter7: Chemical Energy
Section: Chapter Questions
Problem 62E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...
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0.700 moles of an unknown solid is placed into water to make 150.0 mL of solution. The solution's temperature decreases by 7.61°C. Calculate ∆H, in kJ/mol, for the dissolution of the unknown solid. (The specific heat of the solution is 4.184 J/g・°C and the density of the solution is 1.02 g/mL).
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