If the energy needed to break two moles of C=O bonds is greater than the sum of the energies nee

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If the energy needed to break two moles of C=O bonds is...

If the energy needed to break two moles of $\mathrm{C}=\mathrm{O}$ bonds is greater than the sum of the energies needed to break the $\mathrm{O}=\mathrm{O}$ bonds in one mole of $\mathrm{O}_{2}$ and vaporize one mole of carbon, why does the combustion of pure carbon release heat?

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Key Concepts

Bond Energies

Bond energies represent the amount of energy required to break a specific chemical bond, or the energy released when the bond is formed. In any chemical reaction, bonds are broken and formed, and the net energy change depends on the difference between the energy consumed in breaking bonds and the energy released during bond formation.

Reaction Enthalpy

Reaction enthalpy is the overall heat change during a chemical reaction. It is calculated by summing the energies required to break bonds in the reactants and subtracting the energy released when new bonds are formed in the products. Even if certain bond breaking steps require considerable energy, the formation of new, stronger bonds can result in a net release of energy if they release more energy than was consumed.

Chemical Thermodynamics

Chemical thermodynamics, particularly Hess’s law, explains that the total energy change of a reaction is determined by the sum of the energy changes in individual steps. In combustion, although energy is required to break some bonds, the formation of very stable products (with strong bonds) results in an overall exothermic process where the energy released exceeds the energy input, leading to the release of heat.

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