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Given that \( \Delta H_{\mathrm{f}}^{\circ}\left(\mathrm{CO}_{2}, \mathrm{~g}\right)=-393.509 \mathrm{~kJ} \mathrm{~mol}^{-1}, \Delta H_{\mathrm{f}}^{\circ}\left(\mathrm{H}_{2} \mathrm{O}, \mathrm{l}\right)=-285.830 \) \( \mathrm{kJ} \mathrm{mol}^{-1}, \Delta \mathrm{H}_{\mathrm{f}}^{\mathrm{\circ}}\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}, \mathrm{l}\right)=-277.800 \mathrm{~kJ} \mathrm{~mol}^{-1} \).
Calculate the \( \Delta H^{\circ} \) (combustion) of liquid ethanol. The following is the required reaction.
\[
\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(\mathrm{l})+3 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{CO}_{2}(\mathrm{~g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})
\]
(A) \( -1366.82 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
(B) \( -278.82 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
(C) \( -2264.66 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
(D) \( -1155.78 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
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