Assume that the specific heat of the solution is the same as that of pure water. 5.54 (a) When a 3.88-g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature drops from 23.0°C to 18.4°C. Calculate AH (in kJ/mol NH4NO3) for the solu- tion process

Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.62QE: A 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup...
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5.54
Assume that the specific heat of the solution is the same
as that of pure water.
5.54 (a) When a 3.88-g sample of solid ammonium nitrate
dissolves in 60.0 g of water in a coffee-cup calorimeter
(Figure 5.18), the temperature drops from 23.0°C to
18.4°C. Calculate AH (in kJ/mol NH4NO3) for the solu-
tion process
NH4NO3(s) –→ NH4*(aq) + NO3 (aq)
-
Assume that the specific heat of the solution is the same
as that of pure water. (b) Is this process endothermic or
exothermic?
Transcribed Image Text:Assume that the specific heat of the solution is the same as that of pure water. 5.54 (a) When a 3.88-g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature drops from 23.0°C to 18.4°C. Calculate AH (in kJ/mol NH4NO3) for the solu- tion process NH4NO3(s) –→ NH4*(aq) + NO3 (aq) - Assume that the specific heat of the solution is the same as that of pure water. (b) Is this process endothermic or exothermic?
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