Given the bond enthalpies Cl-Cl (243),C-Cl (339),H-Cl (431),C-H (414)all in kJ/mol,estimate ΔH° for the following reaction: CH₄(g)+ Cl₂(g)→ CH₃Cl(g)+ HCl(g). A)-113 kJ/mol B)-356 kJ/mol C)301 kJ/mol D)-1427 kJ/mol E)-30 kJ/mol

Question

Quizplus · Accepted Answer

The ΔH° for the reaction can be estimated using the bond enthalpies given. The bonds broken are one C-H (414 kJ/mol) and one Cl-Cl (243 kJ/mol), and the bonds formed are one C-Cl (339 kJ/mol) and one H-Cl (431 kJ/mol). Thus, ΔH° = (Bonds broken) - (Bonds formed) = (414 + 243) - (339 + 431) = 657 - 770 = -113 kJ/mol.

Given the Bond Enthalpies Cl-Cl (243),C-Cl (339),H-Cl (431),C-H (414)all in KJ/mol,estimate