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Ammonium nitrate (NH₄NO₃), which is found in cold packs, is often used in fertilizers. In cold packs, it reacts with heat from the surroundings in the presence of water to dissociate into ammonium and nitrate ions.

\[ \text{H}_2\text{O} + \text{NH}_4\text{NO}_3 (\text{s}) + \text{heat} \rightarrow \text{NH}_4^+ (\text{aq}) + \text{NO}_3^- (\text{aq}) \]
\[ \Delta H = +28\, \text{kJ} \]

10. If you break open the water packet inside the cold pack and allow the ammonium nitrate and water to mix, you will feel the cold pack becoming cold. Is this reaction spontaneous? Explain, using the definition of spontaneous.

11. Given that the \(\Delta H = +28.0\, \text{kJ}\) for the reaction, is this an example of an exothermic or endothermic reaction? How do you know?

12. Why does the cold pack get cold? Explain your answer in terms of heat flow between the system and the surroundings.

13. Examine the moles of reactants and products and the states of matter for each. Is entropy increasing or decreasing for this reaction? What is the sign of \(\Delta S\)?

14. Find \(\Delta G\) for the above reaction at 298 K using the Gibbs Free energy equation.
\[ \Delta G = \Delta H - (T \cdot \Delta S) \]
\[ \Delta S = +0.107\, \text{kJ/K} \]
\[ \Delta H = +28.0\, \text{kJ} \]

Answer :

Final answer:

Ammonium nitrate in cold packs reacts with water and heat to dissociate into ions, making the pack feel cold. The reaction is spontaneous and endothermic, and the entropy of the system increases. The Gibbs Free Energy for the reaction can be calculated using the Gibbs Free Energy equation.

Explanation:

Ammonium nitrate (NH₄NO₃) is used in cold packs and can dissociate into ammonium and nitrate ions in the presence of water and heat. The reaction is endothermic, meaning it absorbs heat from the surroundings, making the cold pack feel cold. The reaction is spontaneous because it releases heat, which is a driving force for spontaneous processes. The entropy of the system increases because solid NH₄NO₃ dissociates into separate ions in solution, increasing disorder. The Gibbs Free Energy (∆G) for the reaction at 298 K can be found using the equation ∆G = ∆H - (T • ∆S), where ∆H is the enthalpy change and ∆S is the entropy change.

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