Use the molar bond enthalpy data in the table to estimate the value of δh°rxn for the equation? ccl4(g) +2f2(g) -> cf4(g)+2cl2.

(4xC-Cl bond + 2xF-F bond) - (4xC-F bond + 2xCl-Cl bond) 

ΔH°rxn=(4x331 + 2x155) - (4x439 + 2x243) = -608kJ/mol-1

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Molar bond enthalpy is defined as the enthalpy of reaction calculated by the subtraction of standard enthalpies of reactants and enthalpies of the products. The estimate value of for the given equation is -608 kJ/.

Given equation,

Enthalpy for 4 (C-Cl bonds) = 4 x 331 = 1324 joules. Enthalpy for 2 (F - F bonds) = 2 x 155 = 310 joules. Enthalpy for 4 (C - F bonds) = 4 x 439 = 1756 joules.Enthalpy for 2 (Cl - Cl bonds) = 2 x 243 = 486 joules.

Now, molar bond enthalpy:

Therefore, the molar bond enthalpy of the reaction is -608 kJ/.

To know more about molar bond enthalpy, refer to following link:

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