Solved: Calorimetry (Section)(a) When a 4.25-g sample of
Chapter , Problem 56E(choose chapter or problem)
Calorimetry (Section 5.5)
(a) When a 4.25-g sample of solid ammonium nitrate dissolves in of water in a coffee-cup calorimeter (Figure 5.17), the temperature drops from
to \(16.9\ ^{\circ} \mathrm{C}\). Calculate \(\Delta H\) (in \(\mathrm{kJ} / \mathrm{mol}\ \mathrm{NH}_{4} \mathrm{NO}_{3}\)) for the solution process:
\(\mathrm{NH}_{4} \mathrm{NO}_{3}(s) \longrightarrow \mathrm{NH}_{4}^{+}(a q)+\mathrm{NO}_{3}^{-}(a q)\)
Assume that the specific heat of the solution is the same as that of pure water. (b) Is this process endothermic or exothermic?
Equation Transcription:
Text Transcription:
16.9 ^{o}C
H
kJ/mol NH_4NO_3
NH_4NO_3(s){rightarrow}NH_4^+(aq)+NO_3^-(aq)
Unfortunately, we don't have that question answered yet. But you can get it answered in just 5 hours by Logging in or Becoming a subscriber.
Becoming a subscriber
Or look for another answer