Calculate the heat of the following reaction at `25^@C`.
`C_2H_4(g) + H_2(g) to C_2H_6(g)`
The heats of combustion of ethylene, hydrogen and ethane are-1410 kJ, -286.2 kJ and -1560.6 kJ respectively at` 25^@C`.

Explanation

To calculate the heat of the reaction \( C_2H_4(g) + H_2(g) \rightarrow C_2H_6(g) \) at \( 25^\circ C \), we will use the heats of combustion provided for ethylene, hydrogen, and ethane. The heats of combustion are as follows:

- Heat of combustion of ethylene (\( C_2H_4 \)): \( \Delta H = -1410 \, \text{kJ} \)
- Heat of combustion of hydrogen (\( H_2 \)): \( \Delta H = -286.2 \, \text{kJ} \)
- Heat of combustion of ethane (\( C_2H_6 \)): \( \Delta H = -1560.6 \, \text{kJ} \)

### Step 1: Write the combustion reactions
1. **Combustion of ethylene**:
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