Thermochemistry

What is Bond Dissociation Energy (BDE)?

Given the following bond energies: C-H (413 kJ/mol), O=O (498 kJ/mol), C=O (799 kJ/mol), and O-H (463 kJ/mol), what is the enthalpy change for the following reaction? $CH_4(g) + 2O_2(g) ightarrow CO_2(g) + 2H_2O(g)$

Which of the following statements accurately describes the energy changes associated with breaking and forming chemical bonds?

How does the Bond Dissociation Energy (BDE) typically vary between single, double, and triple bonds between the same two atoms?

Consider the following carbon-halogen bonds: C-F, C-Cl, C-Br, and C-I. Rank these bonds in terms of their Bond Dissociation Energies (BDE) from highest to lowest.

Is the following step endothermic or exothermic: $Cl_2(g) ightarrow 2Cl(g)$?

Determine the enthalpy change (ΔH) for the combustion of ethane ($C_2H_6$) to form carbon dioxide and water, given the following average bond enthalpies: C-C = 347 kJ/mol, C-H = 414 kJ/mol, O=O = 498 kJ/mol, C=O = 799 kJ/mol, and O-H = 463 kJ/mol. Note: You will need to determine the balanced chemical equation first.

Given the following approximate bond energies: H-H = 432 kJ/mol, H-Cl = 427 kJ/mol, what is the approximate enthalpy change (ΔH) for the reaction $H_2(g) + Cl_2(g) ightarrow 2HCl(g)$ if the bond energy for Cl-Cl is 242 kJ/mol?