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Problem: Compare the value you obtain using average bond energies to the actual standard enthalpy of formation of gaseous benzene, 82.9 kJ/mol. What does the difference between these two values tell you about the stability of benzene?

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We have to compare the actual enthalpy of formation of gaseous benzene with the enthalpy of formation calculated from average bond energies.


The change in enthalpy when one mole of a substance is formed from its reactants in their standard states, is called standard enthalpy of formation (Δf).


Standard enthalpy of reaction can be calculated using the bond energies:

H°rxn = ΣBEreactants - ΣBEproducts

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Problem Details

Compare the value you obtain using average bond energies to the actual standard enthalpy of formation of gaseous benzene, 82.9 kJ/mol. What does the difference between these two values tell you about the stability of benzene?

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What scientific concept do you need to know in order to solve this problem?

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.