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.
![**Problem Statement:**
The reaction releases 251 kJ of heat. What is the ΔH for the reaction as written? [Input field] kJ/mol
**Explanation:**
This is a thermodynamics problem asking for the enthalpy change (ΔH) of a chemical reaction, measured in kilojoules per mole (kJ/mol). The given data indicates that the reaction releases 251 kJ of heat, which suggests it is exothermic. The task is to calculate or confirm the ΔH for this reaction based on the provided information.
**Instructions:**
Enter your calculated value for ΔH in the input field provided, making sure to include the correct unit of measurement (kJ/mol).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb3cca2f6-99a8-4436-ac34-ddd5c6eac033%2Fbb16eb2f-82a8-4232-916a-dc3449149206%2Frww7isi_processed.png&w=3840&q=75)
![The image presents a chemical reaction involving the combustion of methanol. Here is the transcription suitable for an educational website:
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**Combustion of Methanol:**
In this reaction, 11.08 grams of liquid methanol (\( \text{CH}_3\text{OH} \)) is burned in excess oxygen gas. The reaction can be represented as follows:
\[
2 \, \text{CH}_3\text{OH}(l) + 3 \, \text{O}_2(g) \rightarrow 2 \, \text{CO}_2(g) + 4 \, \text{H}_2\text{O}(l)
\]
**Explanation:**
- **Reactants:**
- Methanol (\( \text{CH}_3\text{OH} \)) is in liquid form.
- Oxygen (\( \text{O}_2 \)) is in gaseous form.
- **Products:**
- Carbon dioxide (\( \text{CO}_2 \)) is in gaseous form.
- Water (\( \text{H}_2\text{O} \)) is in liquid form.
This balanced chemical equation illustrates the complete combustion process of methanol, where two moles of methanol react with three moles of oxygen to produce two moles of carbon dioxide and four moles of water. This type of reaction is exothermic, releasing energy as heat.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb3cca2f6-99a8-4436-ac34-ddd5c6eac033%2Fbb16eb2f-82a8-4232-916a-dc3449149206%2Ffl2950m_processed.png&w=3840&q=75)
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