Question:
One mole of ethanol (C₂H₅OH) was completely burnt in oxygen to form CO₂(g) and H₂O(l). What is the \(\Delta H_f^{\circ}\) (in kJ/mol) for this reaction?
One mole of ethanol (C₂H₅OH) was completely burnt in oxygen to form CO₂(g) and H₂O(l). What is the \(\Delta H_f^{\circ}\) (in kJ/mol) for this reaction?
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Use the standard enthalpies of formation and apply Hess's Law to calculate enthalpy changes for combustion reactions.
Updated On: Jun 6, 2025
- 1921
- -1921
- 1367
- -1367
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The Correct Option is D
Solution and Explanation
The standard enthalpy change of formation for ethanol, CO₂, and H₂O is given. Using Hess's Law, the enthalpy of the combustion reaction is calculated by subtracting the enthalpy of formation of the reactants from the products. The correct value of \(\Delta H_f^{\circ}\) is -1367 kJ/mol.
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