Question
What is the change in enthalpy for the combustion of liquid hexane (C6H14)?
Answers
GPT-4o mini
The change in enthalpy for the combustion of liquid hexane (C₆H₁₄) can be determined using the standard enthalpy of combustion. The balanced chemical equation for the complete combustion of hexane is:
\[ \text{C}_6\text{H}_{14}(l) + 19/2 \text{O}_2(g) \rightarrow 6 \text{CO}_2(g) + 7 \text{H}_2\text{O}(l) \]
The standard enthalpy change of combustion (\( \Delta H_{c}^\circ \)) for hexane can usually be found in thermodynamic tables. For hexane, the standard enthalpy of combustion is approximately:
\[ \Delta H_{c}^\circ \approx -4163 \, \text{kJ/mol} \]
This value indicates that the combustion of 1 mole of hexane releases about 4163 kJ of energy. Please check updated sources or databases for the most accurate and current values, as they can vary slightly between references.
\[ \text{C}_6\text{H}_{14}(l) + 19/2 \text{O}_2(g) \rightarrow 6 \text{CO}_2(g) + 7 \text{H}_2\text{O}(l) \]
The standard enthalpy change of combustion (\( \Delta H_{c}^\circ \)) for hexane can usually be found in thermodynamic tables. For hexane, the standard enthalpy of combustion is approximately:
\[ \Delta H_{c}^\circ \approx -4163 \, \text{kJ/mol} \]
This value indicates that the combustion of 1 mole of hexane releases about 4163 kJ of energy. Please check updated sources or databases for the most accurate and current values, as they can vary slightly between references.