Problem: Use the molar bond enthalpy data in the table to estimate the value of ΔH°rxn for the equationCCI4(g) + 2F2(g) → CF4(g) + 2CI2(g   

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

ΔHrxn = {Bond energy of reactants} - {Bond energy of products}

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

331 x 4 = 1324 kJ/mol

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Use the molar bond enthalpy data in the table to estimate the value of ΔH°rxn for the equation

CCI4(g) + 2F2(g) → CF4(g) + 2CI2(g

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