Calculate the ethalpy of combustion of ethylene (g) to form `CO_(2)` (gas) and `H_(2)O` (gas) at 298 K and 1 atmospheric pressure. The enthalpies of formation of `CO_(2),H_(2)O` and `C_(2)H_(4)` are `-393.7, -241.8+52.3` kJ per mole respectively.

Explanation

To calculate the enthalpy of combustion of ethylene (C₂H₄) to form carbon dioxide (CO₂) and water (H₂O) at 298 K and 1 atmospheric pressure, we will follow these steps:

### Step 1: Write the balanced chemical equation for the combustion of ethylene.
The combustion of ethylene can be represented by the following reaction:

\[ \text{C}_2\text{H}_4(g) + \text{O}_2(g) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(g) \]

Balancing the equation, we get:
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