?Once consumed, the body metabolizes alcohol (ethanol, \(\mathrm{CH}_{3} \mathrm{CH}_{2}
Chapter 7, Problem 7.6(choose chapter or problem)
Once consumed, the body metabolizes alcohol (ethanol, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\); molar mass = 46\( \mathrm{~g} / \mathrm{mol})\) to carbon dioxide and water. The balanced reaction is: \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}+3 \mathrm{O}_{2} \longrightarrow 2 \(\mathrm{CO}_{2}+3 \mathrm{H}_{2} \mathrm{O}\). Using the bond energies in Table 7.1, estimate the \(\Delta H\) for this reaction in \(\mathrm{kJ} / \mathrm{mol}\). How does it compare to the energy value of alcohol \(\mathrm{J} / \mathrm{g})\) given in the Chemistry in Action feature “Energy from Food” on p. 225?
Text Transcription:
CH_3 CH_2 OH
46/~g/mol
CH_3 CH_2 OH+3 O_2 longrightarrow 2
CO_2+3 H_2/O
Delta H
kJ/mol
J/g
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