Bond Dissociation Energies In chemical reactions, heat is converted into chemical energy (the potential energy stored in chemical bonds) or vice versa. Thus, enthalpy change for a reaction can be approximated from ΔH∘=D(reactants)−D(products) where D represents bond dissociation energies of the reactants and products, respectively. The table below contains the bond dissociation energies for common bonds. The information can be used to calculate the energy needed to break all the bonds in a given molecule. Bond Dissociation energy (kJ/mol ) C−C 350 C=C 611 C−H 410 C−O 350 C=O 732 O−O 180 O=O 498 H−O 460 Due to the variation in literature values of thermodynamic quantities: Assume that these values sufficiently represent the bonds in the compounds involved in the following questions Be sure that you use the values given in the table in the introduction for your calculations in this item. Part A Calculate the bond dissociation energy for the breaking of all the bonds in a mole of methane, CH4. Express your answer to four significant figures and include the appropriate units. DCH4 = 1652 kJmol SubmitHintsMy AnswersGive UpReview Part Correct Part B What is the bond dissociation energy for breaking all the bonds in a mole of O2 molecules? Express your answer to three significant figures and include the appropriate units. DO2 = 495 kJmol SubmitHintsMy AnswersGive UpReview Part Correct Part C Calculate the bond dissociation energy required for breaking all the bonds in a mole of water molecules, H2O. Express your answer as an integer and include the appropriate units. DH2O = 926 kJmol SubmitHintsMy AnswersGive UpReview Part Correct Therefore the enthalpy change for forming a mole of water is −920 kJ. This is why D(products) is negative in the equation. Part D Calculate the bond dissociation energy needed to break all the bonds in a mole of carbon dioxide, CO2. Express your answer as an integer and include the appropriate units. DCO2 = 1598 kJmol SubmitHintsMy AnswersGive UpReview Part Correct Therefore the enthalpy change for forming a mole of carbon dioxide is a negative value. This is why D(products) is negative in the equation. Part E Calculate the approximate enthalpy change , ΔH∘, for the combustion of methane: CH4+2O2⇌2H2O+CO2 Use the values you calculated in Parts A to D, keeping in mind the stoichiometric coefficients. Express your answer to three significant figures and include the appropriate units. ΔH∘ =