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.
![The diagram shows the change in energy over the course of a reaction.
### Diagram Analysis
The graph illustrates energy (in kJ/mol) on the y-axis versus the reaction progress on the x-axis. Initially, the energy level is around 120 kJ/mol. As the reaction progresses, the energy increases to approximately 150 kJ/mol, indicating the peak of the energy required for the reaction. After reaching the peak, the energy sharply decreases to approximately 60 kJ/mol, suggesting a release of energy.
### Questions
**1. Is the reaction exergonic or endergonic?**
- [ ] exergonic
- [ ] endergonic
**2. Is ΔG for the reaction positive or negative?**
- [ ] negative
- [ ] positive
**Explanation:**
- *Exergonic Reaction:* If the reaction releases energy, indicated by a final energy level lower than the initial, the reaction is exergonic.
- *Endergonic Reaction:* If the reaction absorbs energy, indicated by a final energy level higher than the initial, the reaction is endergonic.
- *ΔG (Gibbs Free Energy Change):* If negative, the reaction is spontaneous (usually exergonic). If positive, the reaction is non-spontaneous (usually endergonic).
The diagram indicates an exergonic reaction with a negative ΔG, given the energy release at the end.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff32c3ee5-84ad-4b8f-a5ee-9f2098075ae5%2F87173c99-deec-46c7-be8c-4e5ed35f87e7%2F3u11top_processed.jpeg&w=3840&q=75)
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