Estimate the enthalpy of reaction (in kJ/mol) for the combustion of methane. Be sure to show a lewis structure for each molecule. CH, (g) + 20, (g)→ CO, (g) + H,O (g) Bond Bond Enthalpy (kJ/mol) C-O 351 C=0 799 CEO 1070 O-0 142 O=0 498 C-H 414 O-H 460
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.
![### Estimating the Enthalpy of Reaction for Methane Combustion
**Objective:**
Estimate the enthalpy of reaction (in kJ/mol) for the combustion of methane. This will involve drawing the Lewis structures for each molecule involved.
**Chemical Reaction:**
\[ \text{CH}_4(g) + 2\text{O}_2(g) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(g) \]
**Bond Enthalpy Values:**
- C–O: 351 kJ/mol
- C=O: 799 kJ/mol
- C≡O: 1070 kJ/mol
- O–O: 142 kJ/mol
- O=O: 498 kJ/mol
- C–H: 414 kJ/mol
- O–H: 460 kJ/mol
**Steps to Calculate Enthalpy:**
1. **Draw Lewis Structures:**
- Identify the bonds broken and formed in each molecule.
2. **Calculate Total Energy Required to Break Bonds:**
- Sum the bond enthalpies of all bonds broken in the reactants.
3. **Calculate Total Energy Released Forming Bonds:**
- Sum the bond enthalpies of all bonds formed in the products.
4. **Estimate Enthalpy Change:**
- Use the formula:
\[ \Delta H = \text{Energy of bonds broken} - \text{Energy of bonds formed} \]
By using the bond enthalpies provided, you can estimate the total enthalpy change for the combustion reaction. This calculation will provide insight into the energy efficiency and feasibility of methane as a fuel source.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe486ef45-9c28-49a6-849c-e84f93e2f047%2F9e68a34d-fbe2-4edc-9c3a-08799d33d4bd%2Ftkiixc_processed.png&w=3840&q=75)
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