Compounds with carbon-carbon double bond, such as ethylene, `C_(2)H_(4)`, add hydrogen in a reaction called hydrogenation.
`C_(2)H_(4)(g)+H_(2)(g) rarr C_(2)H_(6)(g)`
Calculate enthalpy change for the reaction, using the following combustion data
`C_(2)H_(4)(g) + 3O_(2)(g) rarr 2CO_(2)(g) + 2H_(2)O(g)`, `Delta_("comb")H^(Θ) = -1401 kJ mol^(-1)`
`C_(2)H_(6)(g) + 7//2O_(2)(g)rarr 2CO_(2) (g) + 3H_(2)O(l)`, `Delta_("comb")H^(Θ) = -1550kJ`
`H_(2)(g) + 1//2O_(2)(g) rarr H_(2)O(l)`, `Delta_("comb")H^(Θ) = -286.0 kJ mol^(-1)`

Explanation

To calculate the enthalpy change (ΔH) for the hydrogenation reaction of ethylene (C₂H₄) to ethane (C₂H₆), we can use the provided combustion data for the relevant reactions.

### Step-by-Step Solution:

1. **Write the target reaction**:
We want to find the enthalpy change for the reaction:
\[
\text{C}_2\text{H}_4(g) + \text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g)
...