Given the following reactions N2 (g) + O2 (g) → 2NO (g) 2NO(g) + O2(g) → 2N (g) the enthalpy of reaction for 4NO (g) - 2NO2 (g) + N2 (g) ΔΗ = +180.7 kJ AH =-113.1 kJ
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.
![## Enthalpy of Reactions
**Given the following reactions:**
1. \( \text{N}_2(\text{g}) + \text{O}_2(\text{g}) \rightarrow 2\text{NO}(\text{g}) \hspace{0.5cm} \Delta H = +180.7 \text{kJ} \)
2. \( 2\text{NO}(\text{g}) + \text{O}_2(\text{g}) \rightarrow 2\text{N}_2(\text{g}) \hspace{0.5cm} \Delta H = -113.1 \text{kJ} \)
**Find the enthalpy of reaction for:**
\[ 4\text{NO}(\text{g}) \rightarrow 2\text{NO}_2(\text{g}) + \text{N}_2(\text{g}) \]
### Explanation:
- **First Reaction (1)**: This shows the formation of nitric oxide (NO) from nitrogen (N2) and oxygen (O2) gases. The enthalpy change (ΔH) is positive, indicating that the reaction is endothermic, and the energy absorbed is 180.7 kJ.
- **Second Reaction (2)**: This reaction involves the formation of nitrogen (N2) gas from nitric oxide (NO) and oxygen (O2) gases. The enthalpy change (ΔH) is negative, which indicates that the reaction is exothermic, and the energy released is 113.1 kJ.
**Note**: The image shows textual information as described and does not contain any graphs or diagrams for further explanation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F35780925-5e45-4c26-92de-ecbbabfbfb48%2F24b38272-dab8-4ce2-ab31-d38ef2842b86%2Fmal056vh_processed.jpeg&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
