Use the bond energies in the table to estimate `DeltaH` for this reaction: `CH_(2) = CH_(2) + Cl_(2) rarr CICH_(2) -CH_(2)CI`

Options

A. `DeltaH = 684 kJ`
B. `DeltaH =- 154 kJ`
C. `DeltaH = 189 kJ`
D. `DeltaH = 177 kJ`

Explanation

To estimate the enthalpy change (ΔH) for the reaction \( CH_2=CH_2 + Cl_2 \rightarrow ClCH_2-CH_2Cl \), we will use the bond energies provided in the table. The enthalpy change can be calculated using the formula:

\[ \Delta H = \text{Total bond energy of reactants} - \text{Total bond energy of products} \]

### Step 1: Identify the bonds in the reactants
The reactants are \( CH_2=CH_2 \) (ethene) and \( Cl_2 \) (chlorine gas).
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