In a molecule of methane CH4 , there are four C-H bonds and no C-C bonds. To determine the bond energy required to break all the bonds in a molecule of methane, we will only consider the C-H bond energy.For one molecule of CH4, the total bond energy required to break all C-H bonds is:Total bond energy = Number of C-H bonds x C-H bond energy Total bond energy = 4 x 413 kJ/molTotal bond energy = 1652 kJ/molNow, we need to calculate the total energy required to break all the bonds in 4.0 moles of methane:Total energy = Number of moles x Total bond energy per mole Total energy = 4.0 moles x 1652 kJ/molTotal energy = 6616 kJSo, the total energy required to break all the bonds in 4.0 moles of methane is 6616 kJ.