Use the information below to answer this question. \[ \begin{array}{ll}C(s)+O_{2}(g) \rightarrow \mathrm{CO}_{2}(g) & \Delta H^{\circ}=-393.5 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{H}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) & \Delta H^{\circ}=-285.8 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ 3 \mathrm{C}(\mathrm{s})+4 \mathrm{H}_{2}(g) \rightarrow \mathrm{C}_{3} H_{8}(g) & \Delta H^{\circ}=-104.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ 4 C(s)+5 \mathrm{H}_{2}(g) \rightarrow C_{4} H_{10}(g) & \Delta H^{\circ}=-125.2 \mathrm{~kJ} \mathrm{~mol}^{-1}\end{array} \] What is the value, in \( \mathrm{kJ} \mathrm{mol}^{-1} \), for the enthalpy of combustion of propane, \( C_{3} H_{8} \) ?
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