Given the data below, what approximately is D H for the reaction?
H₂ (g) + C₂H₄ (g) →C₂H₆ (g) Average Bond Energies:
H - H₄36 kJ/mol C - H₄14 kJ/mol C=C₆11 kJ/mol C - C₃48 kJ/mol

Question

Given the data below, what approximately is D H for the reaction? H₂ (g) + C₂H₄ (g)→C₂H₆ (g) Average Bond Energies: H - H₄36 kJ/mol C - H₄14 kJ/mol C=C₆11 kJ/mol C - C₃48 kJ/mol

Quizplus · Accepted Answer

The reaction involves breaking one H-H bond and one C=C bond, and forming two C-H bonds and one C-C bond. The enthalpy change (ΔH) is calculated as: ΔH = [Energy of bonds broken] - [Energy of bonds formed] = [(436 + 611) - (2*414 + 348)] = -129 kJ/mol.

Given the Data Below, What Approximately Is D H for the Reaction