(a) When a 4.25-g sample of solid ammonium nitrate dissolvesin 60.0 g of water in a coffee-cup calorimeter (Figure5.18), the temperature drops from 22.0 to 16.9 °C. CalculateΔH (in kJ>mol NH4NO3) for the solution process:NH4NO31s2¡ NH4+1aq2 + NO3-1aq2Assume that the specific heat of the solution is the sameas that of pure water. (b) Is this process endothermic orexothermic?
(a) When a 4.25-g sample of solid ammonium nitrate dissolvesin 60.0 g of water in a coffee-cup calorimeter (Figure5.18), the temperature drops from 22.0 to 16.9 °C. CalculateΔH (in kJ>mol NH4NO3) for the solution process:NH4NO31s2¡ NH4+1aq2 + NO3-1aq2Assume that the specific heat of the solution is the sameas that of pure water. (b) Is this process endothermic orexothermic?
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) When a 4.25-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 22.0 to 16.9 °C. Calculate
ΔH (in kJ>mol NH4NO3) for the solution process:
NH4NO31s2¡ NH4
+1aq2 + NO3
-1aq2
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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