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Problem: 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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  • To determine the average bond energy of S=O in SO2, we have to calculate the dissociation energy of SO2 and then relate this to the structure of SO2
  • The balanced dissociation of SO2 to gaseous O and S atoms will appear as:

SO2 (g) → S (g) + 2O (g) 

  • The standard heat formation of each species appear as:

ΔHf° (S(g, rhombic)) = 277.2 kJ/mol

ΔHf° (O(g)) = 249.2 kJ/mol

ΔHf° (SO(g)) = -296.8 kJ/mol

  • The energy required for the dissociation (or ΔHrxn) is equal to:

ΔHrxn  =  Σ (ΔHf° (products))  -   Σ (ΔHf° (reactants))

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Problem Details

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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Our tutors have indicated that to solve this problem you will need to apply the Bond Energy concept. If you need more Bond Energy practice, you can also practice Bond Energy practice problems.