CH4(g) gas reacts with F2(g) to produce CH3F(g) and HF(g). b.) Use the bond enthalpies in the table below to calculate a numerical estimate of ΔH for the reaction.

- 484 KJ/mol

Explanation:

The reaction equation is;

CH4(g) + F2 (g) > CH3F(g) + HF(g)

The enthalpy of the reaction can be calculated from bond energies using the formula;

ΔHreaction = Bond energy of reactants - bond energy of products

or

ΔHreaction = Bonds broken - bonds formed

[4(413) + 1(155) - 3(413) + 1(485) + 1(567)]

[(1652 + 155) - (1239 + 485 + 567)]

[1807 - 2291]

= - 484 KJ/mol

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2.4 or just 2

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