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Calculate the enthalpy of formation of ethane from the following data:
(i) \( \mathrm{C}(\mathrm{s})+\mathrm{O}_{2} \) (g) \( \rightarrow \mathrm{CO}_{2} \) (g); \( \Delta_{r} H^{\circ}=-393.5 \mathrm{~kJ} \)
(ii) \( \mathrm{H}_{2} \) (g) \( +\frac{1}{2} \mathrm{O}_{2} \) (g) \( \rightarrow \mathrm{H}_{2} \mathrm{O} \) (l) \( ; \Delta_{r} \mathrm{H}^{\circ}=-285.8 \mathrm{~kJ} \)
(iii)
\[
\begin{array}{r}
\mathrm{C}_{2} \mathrm{H}_{6}(\mathrm{~g})+\frac{7}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{CO}_{2}(\mathrm{~g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \\
\Delta_{r} \mathrm{H}^{\circ}=-1560.0 \mathrm{~kJ}
\end{array}
\]
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