Sorry to keep going on, but I'm assuming you were doing one of those Enthalpy of Reaction questions that require you to use BDE to find the enthalpy. The key thing to realize for those values is that all of those BDE represent the energy required to BREAK a bond (whether its the BDE of a single bond, pi bond, etc). Bonds that are formed release energy. If the overall energy released in forming bonds is greater than the energy input to break the bonds, the reaction will release energy overall and be exothermic. Likewise, if the products release less energy than the energy required to break the bonds, the reaction will consume energy overall and be endothermic.
In this scenario, let's take the same example above: ethyne (HCCH) and somehow react it to produce ethane (H3CCH3). In this scenario, we are breaking two pi bonds in the reactant (HCCH), which consists of a triple bond and producing four new sigma bonds to carbon. Because sigma bonds are always stronger than pi bonds (due to more s characteristic), we can then say that not only will the product be more stable, but it will be exothermic as well (releasing energy in the progress).
Sorry, just wanted to clarify things a bit.