Question
What is the energy change when methane reacts with oxygen?
Answers
GPT-4o mini
The reaction of methane (CH₄) with oxygen (O₂) is a combustion reaction that produces carbon dioxide (CO₂) and water (H₂O). The balanced chemical equation for the complete combustion of methane is:
\[ \text{CH}_4(g) + 2\text{O}_2(g) \rightarrow \text{CO}_2(g) + 2\text{H}_2\text{O}(g) \]
To assess the energy change associated with this reaction, we look at the enthalpy change, or ΔH, which is typically negative for combustion reactions because they release energy. For the combustion of methane, the standard enthalpy change (ΔH) is approximately -890 kJ per mole of methane when combusted completely in excess oxygen.
This negative value indicates that energy is released as heat, making the reaction exothermic. The exact value can vary slightly based on standard conditions and reference sources, but it's generally around -890 kJ/mol.
In summary, the energy change when methane reacts with oxygen in a combustion reaction is exothermic, approximately -890 kJ per mole of methane burned.
\[ \text{CH}_4(g) + 2\text{O}_2(g) \rightarrow \text{CO}_2(g) + 2\text{H}_2\text{O}(g) \]
To assess the energy change associated with this reaction, we look at the enthalpy change, or ΔH, which is typically negative for combustion reactions because they release energy. For the combustion of methane, the standard enthalpy change (ΔH) is approximately -890 kJ per mole of methane when combusted completely in excess oxygen.
This negative value indicates that energy is released as heat, making the reaction exothermic. The exact value can vary slightly based on standard conditions and reference sources, but it's generally around -890 kJ/mol.
In summary, the energy change when methane reacts with oxygen in a combustion reaction is exothermic, approximately -890 kJ per mole of methane burned.