Problem: Complete combustion of 1 mol of acetone (C3H6O) liberates 1790 kJ:C3H6O(l) + 4O2(g) → 3CO2(g) + 3H2O(l)  ΔHo= - 1790Using this information together with the standard enthalpies of formation of O2(g), CO2(g), and H2O(l) from Appendix C, calculate the standard enthalpy of formation of acetone.

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We are asked to calculate the standard enthalpy of formation of acetone


Calculate the enthalpy change for the reaction: C3H6O(l) + 4O2(g) → 3CO2(g) + 3H2O(l)  ΔHo= - 1790



ΔH°rxn=ΔH°f, product-ΔH°f,reactant


Note that we need to multiply each ΔH˚ by the stoichiometric coefficient since ΔH˚ is in kJ/mol. 


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Problem Details

Complete combustion of 1 mol of acetone (C3H6O) liberates 1790 kJ:
C3H6O(l) + 4O2(g) → 3CO2(g) + 3H2O(l)  ΔHo= - 1790

Using this information together with the standard enthalpies of formation of O2(g), CO2(g), and H2O(l) from Appendix C, calculate the standard enthalpy of formation of acetone.

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