From the following data at \(25^{\circ} \mathrm{C}\), calculate the \(\Delta_{\mathrm{r}} \mathrm{H}^0\) for \(\mathrm{H}_2 \mathrm{O}(\mathrm{g}) \rightarrow 2 \mathrm{H}(\mathrm{g})+\mathrm{O}(\mathrm{g})\)
reaction: \(\Delta_{\mathrm{r}} \mathrm{H}^0\left(\mathrm{~kJ} \mathrm{~mol}^{-1}\right)\)
\[
\begin{array}{ll}
\frac{1}{2} \mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{OH}(\mathrm{g}) & 42.09 \\
\mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g}) & -242 \\
\mathrm{H}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g}) & 436 \\
\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{O}(\mathrm{g}) & 496
\end{array}
\]

1. A \(1174 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
2. B \(742 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
3. C \(926 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
4. D \(690 \mathrm{~kJ} \mathrm{~mol}^{-1}\)