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 $\Delta H_{\mathrm{rxn}}$ for the hydrogenation reaction. $$\mathrm{H}_{2} \mathrm{C}=\mathrm{CH}_{2}(g)+\mathrm{H}_{2}(g) \longrightarrow \mathrm{H}_{3} \mathrm{C}-\mathrm{CH}_{3}(g)$$

Hydrogenation reactions are used to add hydrogen across double bonds in hydrocarbons and other organic compounds. Use average bond energies to calculate $\Delta H_{\mathrm{rxn}}$ for the hydrogenation reaction.
$$\mathrm{H}_{2} \mathrm{C}=\mathrm{CH}_{2}(g)+\mathrm{H}_{2}(g) \longrightarrow \mathrm{H}_{3} \mathrm{C}-\mathrm{CH}_{3}(g)$$

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Key Concepts

Hydrogenation Reaction

A hydrogenation reaction is a process in which hydrogen is added to unsaturated compounds, converting double or triple bonds into single bonds. This type of reaction is fundamental in organic chemistry and industrial applications, as it is used to alter the saturation and properties of organic molecules.

Average Bond Energies

Average bond energies are representative values for the energy required to break a particular type of bond in various molecules. They provide a useful approximation for determining the energy changes in reactions when precise bond energies are not available.

Bond Breaking and Bond Formation

The calculation of a reaction's enthalpy change involves assessing the energy required to break bonds in the reactants and the energy released when new bonds are formed in the products. This concept is essential for understanding energy profiles in chemical reactions.

Reaction Enthalpy (?H_rxn)

Reaction enthalpy (?H_rxn) is the measure of heat absorbed or released during a chemical reaction at constant pressure. It is calculated by subtracting the total energy released in forming bonds from the total energy consumed in breaking bonds, thereby indicating whether the reaction is exothermic or endothermic.

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