Using the Heat of Combustion of Methanol as -726

Using the heat of combustion of methanol as -726.6 kJ and the following data: C(graph) + 1/2O₂ → CO(g)  ΔH° = -110.5 kJ
C(graph) + O₂(g) → CO₂(g)  ΔH° = -393.5 kJ
H₂(g) + 1/2O₂(g) → H₂O(l)  ΔH° = -285.8 kJ
Determine ΔH° for the following reaction:
CO(g) + 2 H₂(g) → CH₃OH(l)

A) -349 kJ
B) 157.8 kJ
C) -157.8 kJ
D) 128 kJ
E) -128 kJ