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Problem: Hydrogenation reactions are used to add hydrogen across double bonds in hydrocarbons and other organic compounds. Use average bond energies to calculate ΔHrxn for the following hydrogenation reaction: H2C=CH2(g) + H2(g) → H3C–CH3(g)

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Hrxn = Hbond reactants - Hbond productsHrxn =[4(C-H) + 1(C=C) + 1(H-H)] - [6(C-H) + 1(C-C)]Hrxn =[4 mol C-H (413 kJ1 mol C-H) + 1 mol C=C (612 kJ 1 mol C=C) + 1 mol H-H(436 kJ1 mol H-H)]                   - [6 mol C-H 413 kJ1 mol C-H + 1 mol C-C347 kJ1 mol C-C]


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Problem Details

Hydrogenation reactions are used to add hydrogen across double bonds in hydrocarbons and other organic compounds. Use average bond energies to calculate ΔHrxn for the following hydrogenation reaction: H2C=CH2(g) + H2(g) → H3C–CH3(g)

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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.

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Based on our data, we think this problem is relevant for Professor Russell's class at UNCG.