Given that ΔH° = -311 kJ for the hydrogenation of acetylene, C₂H₂: H-C≡C-H(g) + 2 H₂(g) → CH₃-CH₃(g) and the following bond dissociation energies: H-H = 436 kJ/mol, C-H = 413 kJ/mol, and C-C = 348 kJ/mol, estimate a value for the C≡C triple bond dissociation energy?

Ethane, C2H6, is an alkane with one C─C bond and six C─H bonds (Section 2.9). a. Use enthalpies of formation given in Appendix C to calculate Δ𝐻 for the reaction C2H6(𝑔)→2C(𝑔)+6H(𝑔). b. Use the result from part (a) and the value of 𝐷(C─H) from Table 5.4 to estimate the bond enthalpy 𝐷(C─C). c. How large is the difference between the value calculated for in part (b) and the value given in Table 5.4?

Use average bond enthalpies from Table 5.4 to estimate Δ𝐻 for the following gas-phase reaction of ethylene, (C2H4), oxygen, and hydrogen to form ethylene glycol (C2H6O2), which is the principal component of automotive antifreeze: