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.
![### Balancing Chemical Equations
**Question 4 of 20**
**Task:**
Balance the following chemical equation (if necessary):
\[ \text{C}_3\text{H}_6\text{O}_2(g) + \text{O}_2(g) \rightarrow \text{H}_2\text{O}(g) + \text{CO}_2(g) \]
**Interface Details:**
- **Buttons Available:**
- Numeric buttons (0-9)
- Element and molecule buttons (\(\text{C}_3\text{H}_6\text{O}_2\), \(\text{CO}_2\), \(\text{O}_2\), \(\text{H}_2\text{O}\))
- State buttons (\((s)\), \((l)\), \((g)\), \((aq)\))
- Mathematical and navigation symbols (+, \(\rightarrow\), etc.)
- Special buttons (Reset, arrow keys for navigation)
**Instructions:**
Use the interface to enter coefficients in front of the compounds to balance the chemical equation. Adjust the quantities so that the number of atoms of each element is equal on both sides of the equation.
### Explanation:
In chemical equations, it is crucial to have the same number of atoms of each element on both sides of the reaction arrow. Balancing ensures the law of conservation of mass is observed. Use the provided buttons to update the equation iteratively.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F38543b38-0ca2-4898-a226-639f5edfcbc9%2F357d269a-4b7e-466e-ba01-79ab23d0a517%2F7w55rhk_processed.jpeg&w=3840&q=75)
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