Ammonia burns in the presence of a platinum catalyst to produce nitric oxide, NO: 4 NH, (g) + 50, (g) 4 NO(g) + 6 H,O(g) What is the heat of reactiorfin kJ mol 1 for the reaction above using the following data? Reaction AH (kJ mol¯') 180.6 N2(g) + O2(g) → 2 NO(g) N2(g) + 3 H2(g) → 2 NH3(g) -91.8 -483.7 2 H2(g) + O2(g) → 2 H20(g) Enter your value in the first box and an appropriate unit of measure in the second box. A/
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
![### Heat of Reaction Calculation
#### Problem Statement
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Ammonia burns in the presence of a platinum catalyst to produce nitric oxide, NO:
\[ 4 \text{NH}_3(g) + 5 \text{O}_2(g) \rightarrow 4 \text{NO}(g) + 6 \text{H}_2\text{O}(g) \]
What is the heat of reaction in kJ mol⁻¹ for the reaction above using the following data?
#### Data Table
| Reaction | \(\Delta H\) (kJ mol⁻¹) |
|---------------------------------------------|--------------------------|
| \(\text{N}_2(g) + \text{O}_2(g) \rightarrow 2 \text{NO}(g)\) | 180.6 |
| \(\text{N}_2(g) + 3 \text{H}_2(g) \rightarrow 2 \text{NH}_3(g)\) | -91.8 |
| \(2 \text{H}_2(g) + \text{O}_2(g) \rightarrow 2 \text{H}_2\text{O}(g)\) | -483.7 |
#### Instructions
Enter your value in the first box and an appropriate unit of measure in the second box.
(Note: Show all intermediate steps and final answers clearly on your paper to ensure accurate grading and understanding of the process.)
#### Interactive Input Fields
(These fields are intended for student answers)
- **Calculated value**: \[ \Box \]
- **Unit of measure**: \[ \Box \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb21ffba4-460f-41d0-866e-5be939c02582%2Fab9e2995-10c9-4240-839b-3ec7f8d0e339%2Fy8k1zo_processed.jpeg&w=3840&q=75)
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