Calculate \(\Delta H\) in \(\mathrm{kJ}\) for the following reaction \[ \mathrm{C}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{CO}_2(\mathrm{~g}) \] Given that, \[ \begin{gathered} \mathrm{H}_2 \mathrm{O}(g)+\mathrm{C}(g) \longrightarrow \mathrm{CO}(g)+\mathrm{H}_2(g) ; \ \Delta H=+131 \mathrm{~kJ} \ \mathrm{CO}(g)+\frac{1}{2} \mathrm{O}_2(g) \longrightarrow \mathrm{CO}_2(g) ; \ \Delta H=-282 \mathrm{~kJ} \ \mathrm{H}_2(g)+\frac{1}{2} \mathrm{O}_2(g) \longrightarrow \mathrm{H}_2 \mathrm{O}(g) ; \ \Delta H=-242 \mathrm{~kJ} \end{gathered} \]

1. A \(-393\)
2. B \(+393\)
3. C \(+655\)
4. D \(-655\)