SO2 (g) → S (g) + 2O (g)
ΔHf° (S(g, rhombic)) = 277.2 kJ/mol
ΔHf° (O(g)) = 249.2 kJ/mol
ΔHf° (SO2 (g)) = -296.8 kJ/mol
ΔHrxn = Σ (ΔHf° (products)) - Σ (ΔHf° (reactants))
The standard state of sulfur is solid rhombic sulfur. Use the appropriate standard heats of formation given in Appendix II in the textbook to find the average bond energy of the S=O in SO2.
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