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.
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![For the combustion of methane reaction, how many moles of H₂O can be produced from 1.30 moles of methane (CH₄)? Assume you have an unlimited supply of O₂.
\[ \text{CH}_4 (g) + 2 \text{O}_2 (g) \rightarrow \text{CO}_2 (g) + 2 \text{H}_2\text{O} (g) \]
**Explanation of the Chemical Equation:**
The balanced chemical equation depicts the combustion of methane.
- **Reactants:**
- Methane (\(\text{CH}_4\)) in the gaseous state.
- Oxygen (\(\text{O}_2\)) in the gaseous state, with a stoichiometric coefficient of 2, indicating that two moles of oxygen react with one mole of methane.
- **Products:**
- Carbon dioxide (\(\text{CO}_2\)) in the gaseous state, produced in a 1:1 ratio with methane.
- Water (\(\text{H}_2\text{O}\)) in the gaseous state, with a stoichiometric coefficient of 2, indicating that two moles of water are formed per mole of methane reacted.
**Calculation:**
According to the balanced equation, 1 mole of methane produces 2 moles of water. Therefore, 1.30 moles of methane will produce:
\[ 1.30 \, \text{moles CH}_4 \times \frac{2 \, \text{moles H}_2\text{O}}{1 \, \text{mole CH}_4} = 2.60 \, \text{moles H}_2\text{O} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F463bcd6d-f181-445e-b06b-62a60ab90171%2F5cea94f3-eb91-46c1-8d18-5f108f9e7c00%2Fb45vqvc_processed.png&w=3840&q=75)
In combustion reaction of methane one mole of methane react with two mole of oxygen and produced two mole of water and one mole of carbon dioxide
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