Final answer:
The average bond enthalpies of all triple bonds are not the same; they vary based on the atoms involved, making the statement false.
Step-by-step explanation:
The statement that the average bond enthalpies of all triple bonds are the same value regardless of what atoms are involved is false. While it is true that triple bonds are generally stronger than double or single bonds, the strength of a bond, and thus its bond enthalpy, varies depending on the atoms involved.
For example, a carbon-carbon triple bond has a different bond enthalpy than a nitrogen-nitrogen triple bond. Bond enthalpies are influenced by several factors including the size of the atoms and the number of electron pairs shared between them. For instance, C-F bonds have a different bond enthalpy compared to C-Cl bonds due to differences in electronegativity and atomic size.