$$\ce{CO(g) + 2H(g) <--> CH3OH(g)} \hskip{2em} \Delta H \lt 0$$

Which of the following statements is true about bond energies in this reaction?

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Energy is absorbed in order to break bonds. Energy is released when bonds are formed.

Enthalpy is related to bond formation and breaking by:

$$\Delta H = \sum \Delta H_{\text{bonds broken}} - \sum \Delta H_{\text{bonds formed}}$$

Since $\Delta H$ is negative,

$$\Delta H \lt 0$$ $$\sum \Delta H_{\text{bonds broken}} - \sum \Delta H_{\text{bonds formed}} \lt 0$$ $$\sum \Delta H_{\text{bonds broken}} \lt \sum \Delta H_{\text{bonds formed}}$$