Using the bond energies provided below, calculate $\Delta$ H° for the reaction CH₄(g) + 4Cl₂(g) $\to$ CCl₄(g) + 4HCl(g)
Bond energies: C-H = 413 kJ/mol, Cl-Cl = 243 kJ/mol, C-Cl = 339 kJ/mol, H-Cl = 427 kJ/mol

Question

Using the bond energies provided below, calculate

\Delta

H° for the reaction CH₄(g) + 4Cl₂(g)

\to

CCl₄(g) + 4HCl(g)
Bond energies: C-H = 413 kJ/mol, Cl-Cl = 243 kJ/mol, C-Cl = 339 kJ/mol, H-Cl = 427 kJ/mol

Quizplus · Accepted Answer

The reaction involves breaking 4 C-H bonds and 4 Cl-Cl bonds, and forming 4 C-Cl bonds and 4 H-Cl bonds. The energy change is calculated as: (4 * 413 + 4 * 243) - (4 * 339 + 4 * 427) = 2624 - 3064 = -440 kJ.

Using the Bond Energies Provided Below, Calculate Δ\DeltaΔ H° for the Reaction CH4(g) + 4Cl2(g)

Using the Bond Energies Provided Below, Calculate $\Delta$ H° for the Reaction CH₄(g) + 4Cl₂(g)