Using the table of average bond energies below,the ΔH for the reaction is ________ kJ. H-C≡C-H (g) + H-Cl (g) → H₂C CHCl (g)
Bond: C≡C C=C H-Cl C-Cl C-H
D (kJ/mol) : 839 614 431 328 413

Question

Using the table of average bond energies below,the ΔH for the reaction is ________ kJ. H-C≡C-H (g) + H-Cl (g) → H₂C

CHCl (g)
Bond: C≡C C=C H-Cl C-Cl C-H
D (kJ/mol) : 839 614 431 328 413

Quizplus · Accepted Answer

To calculate the ΔH for the reaction, we need to calculate the total bond energies of the bonds broken and the bonds formed.

Bonds Broken:
1 H-C≡C bond = 839 kJ/mol
1 H-Cl bond = 431 kJ/mol

Bonds Formed:
1 C-H bond = 413 kJ/mol
1 C-Cl bond = 328 kJ/mol
1 C=C bond = 614 kJ/mol

Total Bond Energies Broken - Total Bond Energies Formed = ΔH
(1 x 839) + (1 x 431) - (1 x 413) - (1 x 328) - (1 x 614) = -85 kJ/mol

Therefore, the answer is B) -85.

Using the Table of Average Bond Energies Below,the ΔH for the Reaction