AP Chemistry
6.6 Introduction to Enthalpy of Reaction
6.4 Heat Capacity and Calorimetry
A student adds \(8.00\text{ g}\) of solid ammonium nitrate, \(\text{NH}_4\text{NO}_3\) (molar mass \(80.0\text{ g/mol}\)), to \(92.0\text{ g}\) of distilled water at \(25.0^\circ\text{C}\) inside an insulated coffee-cup calorimeter. The solid dissolves completely according to the equation below, and the temperature of the resulting solution decreases to a minimum of \(19.0^\circ\text{C}\).
\[ \text{NH}_4\text{NO}_3\text{(s)} \rightarrow \text{NH}_4^+\text{(aq)} + \text{NO}_3^-\text{(aq)} \]
Assuming the solution has a specific heat capacity of \(4.18\text{ J}/(\text{g}\cdot^\circ\text{C})\) and that heat transfer with the calorimeter walls and surroundings is negligible, what is the experimental molar enthalpy of solution, \(\Delta H_{\text{soln}}\), for \(\text{NH}_4\text{NO}_3\)?
\[ \text{NH}_4\text{NO}_3\text{(s)} \rightarrow \text{NH}_4^+\text{(aq)} + \text{NO}_3^-\text{(aq)} \]
Assuming the solution has a specific heat capacity of \(4.18\text{ J}/(\text{g}\cdot^\circ\text{C})\) and that heat transfer with the calorimeter walls and surroundings is negligible, what is the experimental molar enthalpy of solution, \(\Delta H_{\text{soln}}\), for \(\text{NH}_4\text{NO}_3\)?
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