# Problem: Use the molar bond enthalpy data in the table to estimate the value of change in Hrxn for the equation: CCl4 (g) + 2 F2 (g) yields CF4 (g) + 2 Cl2 (g). Average Molar bond enthalpies: (C-Cl) = 331 kJ/mol; (F-F) = 155 kJ/mol; (C-F) = 439 kJ/mol; (Cl-Cl) = 243 kJ/mol.

###### FREE Expert Solution
91% (468 ratings)
###### FREE Expert Solution

To find the enthalpy of formation in terms of bond energies, use the equation:

$\Delta H_{rxn} = Bond \; energy\; of\; reactants - Bond \; energy \; of \; products$

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The first reactant has 4 C-Cl bonds. Each C-Cl bond has a bond enthalpy of $331 kJ/mol.$

91% (468 ratings) ###### Problem Details

Use the molar bond enthalpy data in the table to estimate the value of change in Hrxn for the equation: CCl(g) + 2 F(g) yields CF(g) + 2 Cl(g). Average Molar bond enthalpies: (C-Cl) = 331 kJ/mol; (F-F) = 155 kJ/mol; (C-F) = 439 kJ/mol; (Cl-Cl) = 243 kJ/mol.

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Based on our data, we think this problem is relevant for Professor Keene's class at MERCER.