Hydrogenation reactions are used to add hydrogen across...

Hydrogenation reactions are used to add hydrogen across double bonds in hydrocarbons and other organic compounds. Use average bond energies to calculate $\Delta H_{\text {tan }}$ for the hydrogenation reaction. MISSED THIS? Read Section 10.10 ; Watch ME 10.11 $\mathrm{H}_{2} \mathrm{C}=\mathrm{CH}_{2}(\mathrm{~g})+\mathrm{H}_{2}(g) \longrightarrow \mathrm{H}_{3} \mathrm{C}-\mathrm{CH}_{3}(g)$

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Key Concepts

Hydrogenation Reaction

A hydrogenation reaction is a process in which hydrogen (H?) is added across unsaturated bonds, such as carbon-carbon double bonds, converting alkenes or alkynes into more saturated compounds like alkanes. This type of reaction is significant in both organic synthesis and industrial applications for modifying molecular structures to alter physical and chemical properties.

Average Bond Energies

Average bond energies provide an approximate measure of the strength of a chemical bond by indicating the energy required to break one mole of a specific bond type in the gas phase. They are useful in thermochemical calculations where precise bond energies are not known, allowing for the estimation of reaction enthalpies through a simplified and generalized approach.

Bond Enthalpy Calculation

The bond enthalpy calculation is an application of the concept that the overall enthalpy change (?H) of a reaction can be estimated by subtracting the energy released when new bonds form from the energy required to break the bonds present in the reactants. This method relies on summing the relevant average bond energies for all bonds broken and formed, thereby providing insights into the energy profile of chemical reactions such as hydrogenation.

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