The reaction between nitrogen and oxygen is given below: N2(g) + 2 O2(g) → 2 NO2(g) We therefore know that which of the following reactions can also occur? 2 N20(g) → 2 N2(g) + O2(g) N20(g) → 2 NH3(g) + 2 O2(g) O2 N2(g) + O2(g) → 2 N20(g) None of the Above
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.
![### Understanding Nitrogen and Oxygen Reactions
The reaction between nitrogen and oxygen is given below:
\[ \text{N}_2(g) + 2 \text{O}_2(g) \rightarrow 2 \text{NO}_2(g) \]
Having this information, we can determine which of the following chemical reactions can also occur based on the given equation:
1. \[ 2 \text{N}_2\text{O}(g) \rightarrow 2 \text{N}_2(g) + \text{O}_2(g) \]
2. \[ \text{N}_2\text{O}(g) \rightarrow 2 \text{NH}_3(g) + 2 \text{O}_2(g) \]
3. \[ 2 \text{N}_2(g) + \text{O}_2(g) \rightarrow 2 \text{N}_2\text{O}(g) \]
4. None of the Above
In these options:
- The first option describes the decomposition of nitrous oxide into nitrogen and oxygen.
- The second option shows the formation of ammonia and oxygen from nitrous oxide.
- The third option shows the formation of nitrous oxide from nitrogen and oxygen.
Evaluate the given reactions considering the provided nitrogen and oxygen reaction to determine their feasibility.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbc7db68c-7828-4a06-bc34-18cdd71bf49b%2F2c2c26a7-0078-4c33-93f3-7cc38d158db5%2Fvpwy2z_processed.png&w=3840&q=75)
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