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.
Calculate ΔHrxnΔHrxn for the following reaction:
BaO(s)+CO2(g)→BaCO3(s)
Use the following reactions and the given values of ΔHΔH for them:
![### Thermochemistry of Barium Reactions
Consider the following two reactions involving barium (Ba):
1. **Formation of Barium Carbonate:**
\[ \text{Ba(s)} + \text{CO}_2(\text{g}) + \frac{1}{2}\text{O}_2(\text{g}) \rightarrow \text{BaCO}_3(\text{s}), \quad \Delta H = -826.5 \, \text{kJ} \]
2. **Formation of Barium Oxide:**
\[ 2\text{Ba(s)} + \text{O}_2(\text{g}) \rightarrow 2\text{BaO(s)}, \quad \Delta H = -1184.0 \, \text{kJ} \]
### Explanation
**Barium Carbonate Formation Reaction:**
- Reactants: Barium solid (\(\text{Ba}\)), Carbon Dioxide gas (\(\text{CO}_2\)), and Oxygen gas (\(\text{O}_2\)).
- Product: Barium Carbonate solid (\(\text{BaCO}_3\)).
- Enthalpy change (\(\Delta H\)): -826.5 kJ (This indicates an exothermic reaction where heat is released into the surroundings).
**Barium Oxide Formation Reaction:**
- Reactants: Barium solid (\(\text{Ba}\)) and Oxygen gas (\(\text{O}_2\)).
- Product: Barium Oxide solid (\(\text{BaO}\)).
- Enthalpy change (\(\Delta H\)): -1184.0 kJ (This also indicates an exothermic reaction where heat is released into the surroundings).
### Understanding the Enthalpy Changes
- The negative sign in \(\Delta H\) for both reactions indicates that these reactions release heat, making them exothermic.
- The enthalpy change (\(\Delta H\)) for the formation of barium oxide is significantly greater than for the formation of barium carbonate, indicating that more energy is released during the formation of barium oxide.
### Application
These reactions are significant in various industrial and chemical processes where understanding the energy release can help in optimizing conditions for efficiency and safety.
#### Graphical Explanation
While there are no graphs or diagrams provided in the image, for an educational website, it would be useful to include:
- **Energy Diagrams:** Visual](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff89f5582-9fdc-4ede-82bb-28c01b8ca835%2Fd2d642ec-7374-4d96-892d-2e14a271f3f9%2F4rmfeocg_processed.png&w=3840&q=75)
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