?Complete combustion of 1 mol of acetone \(\left(\mathrm{C}_{3} \mathrm{H}_{6}
Chapter 5, Problem 5.75(choose chapter or problem)
Complete combustion of 1 mol of acetone \(\left(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\right)\) liberates 1790 kJ :
\(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}(l)+4 \mathrm{O}_{2}(g) \longrightarrow 3 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l) \Delta H^{\circ}=-1790 \mathrm{~kJ}\)
Using this information together with the standard enthalpies of formation of \(\mathrm{O}_{2}(g), \mathrm{CO}_{2}(g)\), and \(\mathrm{H}_{2} \mathrm{O}(l)\) from Appendix C, calculate the standard enthalpy of formation of acetone.
Text Transcription:
(C3H6O)
C3H6O(l) + 4 O2(g) \longrightarrow 3 CO2(g) + 3 H2O(l) \Delta H^{\circ} = -1790 kJ
O2(g), CO2(g)
H2O(l)
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