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The enthalpy change for the following reaction is -802 kJ. Using bond energies, estimate the C-H bond energy in [tex]CH_4(g)[/tex].

\[ CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(g) \]

Options:
A. -402 kJ/mol
B. -100.5 kJ/mol
C. -201 kJ/mol
D. -50.25 kJ/mol

Answer :

Final answer:

The average C-H bond energy in CH4(g) is 415 kJ/mol because there are four moles of C-H bonds broken per mole of the reaction. Although the four C-H bonds are equivalent in the original molecule, they do not each require the same energy to break; once the first bond is broken (which requires 439 kJ/mol), the remaining bonds are easier to break. The 415 kJ/mol value is the average, not the exact value required to break any one bond.

Explanation:

The bond enthalpies in Table T3 allows us to calculate ΔH because 2 C=O and 2 C-O bonds are formed:
AH ≈ 2 mol (-192.0 kJ mol-¹) + 2 mol (-85.5) = -555 kJ

The average C-H bond energy, Dc-H, is 415 kJ/mol because there are four moles of C-H bonds broken per mole of the reaction. Although the four C-H bonds are equivalent in the original molecule, they do not each require the same energy to break; once the first bond is broken (which requires 439 kJ/mol), the remaining bonds are easier to break. The 415 kJ/mol value is the average, not the exact value required to break any one bond.

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