I was recently learning average bond enthalpies and was wondering if it varies at different temperatures. I know that in different molecular configurations, bond strength is affected by the arrangement of the atoms, but at higher temperatures, there is higher vibrational energy, right? So, if we were to compare the C-H bonds in methane at 273.15 K vs 300 K, would we find significant or trivial difference in their respective bond enthalpies? Would the reasoning be because of the additional vibrational energy or is there another factor in play (e.g. increased Van der Waals forces allow for easier breaking of bonds)?