Determine the enthalpy change for the given reaction.
`CH_(4) (g) + Cl_(2) (g) rightarrow CH_(3) Cl(g) + HCI (g)`
Bond energies are given as follows:
`C-H = 412 kJ mol^(-1)`
`C-CI = 338 kJ mol^(-1)`
`CI-CI = 242 kJ mol^(-1)`
`H-CI = 431 kJ mol^(-1)`.

Explanation

To determine the enthalpy change for the reaction:

\[ \text{CH}_4(g) + \text{Cl}_2(g) \rightarrow \text{CH}_3\text{Cl}(g) + \text{HCl}(g) \]

we will use the bond energies provided to calculate the total energy required to break the bonds in the reactants and the total energy released when forming the bonds in the products.

### Step 1: Identify the bonds broken in the reactants
In the reactants, we have:
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