Question
Ammonium nitrate dissolves in water via the following reaction:
N*H_{4}*N*O_{3}(s) -> N * H_{4} ^ (aq) + N*O_{3} ^ (- (aq))
The bond energies of the compounds in the reaction are as follows:
N*H_{4}*N*O_{3} = 3040kJ / m * ol
• NH 4 ^ + = 1564kJ / m * ol
NO 3 ^ - = 1009kJ / m * ol
How much total energy does the reaction have, and how will the environment change when the reaction occurs?
(1 point)
467kJ / m * ol gain heat
467kJ / m * ol lose heat
- 467kJ / m * ol gain heat
- 467kJ / m * ol lose heat
N*H_{4}*N*O_{3}(s) -> N * H_{4} ^ (aq) + N*O_{3} ^ (- (aq))
The bond energies of the compounds in the reaction are as follows:
N*H_{4}*N*O_{3} = 3040kJ / m * ol
• NH 4 ^ + = 1564kJ / m * ol
NO 3 ^ - = 1009kJ / m * ol
How much total energy does the reaction have, and how will the environment change when the reaction occurs?
(1 point)
467kJ / m * ol gain heat
467kJ / m * ol lose heat
- 467kJ / m * ol gain heat
- 467kJ / m * ol lose heat
Answers
GPT-4o mini
To determine how much energy is associated with the dissolution of ammonium nitrate in water, we can use the provided bond energies. The process of dissolving ammonium nitrate can be represented by calculating the energy associated with breaking the bonds in the solid ammonium nitrate and the energy associated with forming the bonds in the aqueous ions (\(NH_4^+\) and \(NO_3^-\)).
**Given bond energies:**
- Energy of \(NH_4NO_3\): 3040 kJ/mol (energy required to break the bonds)
- Energy of \(NH_4^+\): 1564 kJ/mol (energy released when formed)
- Energy of \(NO_3^-\): 1009 kJ/mol (energy released when formed)
**Calculate the total energy change:**
1. Energy required to break the bonds in \( NH_4NO_3 \) (which is endothermic):
- Total energy to break bonds = +3040 kJ/mol (due to dissolution)
2. Energy released when forming \( NH_4^+ \) and \( NO_3^- \) (which is exothermic):
- Total energy released = Energy of \( NH_4^+ \) + Energy of \( NO_3^- \)
- Total energy released = 1564 kJ/mol + 1009 kJ/mol = 2573 kJ/mol (this energy is released, thus negative)
3. Now, calculate the total energy change for the dissolution:
\[
\text{Total energy change} = \text{Energy required to break bonds} - \text{Energy released}
\]
\[
\text{Total energy change} = 3040 \, \text{kJ/mol} - 2573 \, \text{kJ/mol} = 467 \, \text{kJ/mol}
\]
Since the total energy change is positive (+467 kJ/mol), it means that the process is endothermic; heat is absorbed from the surroundings.
Thus, the final answer is:
**467 kJ/mol gain heat.**
**Given bond energies:**
- Energy of \(NH_4NO_3\): 3040 kJ/mol (energy required to break the bonds)
- Energy of \(NH_4^+\): 1564 kJ/mol (energy released when formed)
- Energy of \(NO_3^-\): 1009 kJ/mol (energy released when formed)
**Calculate the total energy change:**
1. Energy required to break the bonds in \( NH_4NO_3 \) (which is endothermic):
- Total energy to break bonds = +3040 kJ/mol (due to dissolution)
2. Energy released when forming \( NH_4^+ \) and \( NO_3^- \) (which is exothermic):
- Total energy released = Energy of \( NH_4^+ \) + Energy of \( NO_3^- \)
- Total energy released = 1564 kJ/mol + 1009 kJ/mol = 2573 kJ/mol (this energy is released, thus negative)
3. Now, calculate the total energy change for the dissolution:
\[
\text{Total energy change} = \text{Energy required to break bonds} - \text{Energy released}
\]
\[
\text{Total energy change} = 3040 \, \text{kJ/mol} - 2573 \, \text{kJ/mol} = 467 \, \text{kJ/mol}
\]
Since the total energy change is positive (+467 kJ/mol), it means that the process is endothermic; heat is absorbed from the surroundings.
Thus, the final answer is:
**467 kJ/mol gain heat.**