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.
![**Title: Calculating Standard Enthalpy Change Using Standard Heats of Formation**
**Introduction**
In this exercise, we aim to calculate the standard enthalpy change for a given chemical reaction using standard heats of formation.
**Chemical Reaction**
\[ 2\text{H}_2\text{S(g)} + 3\text{O}_2\text{(g)} \rightarrow 2\text{H}_2\text{O(g)} + 2\text{SO}_2\text{(g)} \]
**Objective**
Calculate the standard enthalpy change (\(\Delta H^\circ\)) for the reaction.
**Procedure**
1. **Identify Reactants and Products:**
- Reactants: \(\text{H}_2\text{S(g)}\), \(\text{O}_2\text{(g)}\)
- Products: \(\text{H}_2\text{O(g)}\), \(\text{SO}_2\text{(g)}\)
2. **Use Standard Heat of Formation Values:**
- Obtain the standard heat of formation (\(\Delta H_f^\circ\)) for each substance from a reference table.
3. **Apply Hess's Law:**
- Use the equation:
\[
\Delta H^\circ = \sum \Delta H_f^\circ \text{(products)} - \sum \Delta H_f^\circ \text{(reactants)}
\]
4. **Calculate and Fill Out:**
- Calculate using the enthalpy values and fill in the box with the final result in kilojoules (kJ).
**Conclusion**
By following these steps and applying the standard heats of formation, you will determine the standard enthalpy change for the reaction. Fill in the calculated value in the provided box.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9aca1772-1e0c-4e24-86a8-736d39b6760d%2F1f3997cf-9b1a-4cc6-86b0-c571d305596c%2Fdksbm6_processed.jpeg&w=3840&q=75)
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