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

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,

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