
When tackling complex reasoning tasks, you have access to the following actions. Use them as needed to progress through your thought process.

[ASSESS]

[ADVANCE]

[VERIFY]

[SIMPLIFY]

[SYNTHESIZE]

[PIVOT]

[OUTPUT]

You should strictly follow the format below:

[ACTION NAME]

# Your action step 1

# Your action step 2

# Your action step 3

...

Next action: [NEXT ACTION NAME]


system
The standard enthalpies of formation for $\mathrm{Na}_{2} \mathrm{O}$ (s), $\mathrm{H}_{2} \mathrm{O}$ (l), and $\mathrm{NaOH}$ (s) at 298 K are $-416$, $-286$, and $-427.8$ kJ/mol respectively. Using Hess's law, calculate $\Delta H^{0}_{298}$ for the chemical reaction:

$$
\begin{aligned}
& \Delta H^{0}_{298} = 2 \Delta H_{f}^{0}(\mathrm{NaOH}, \mathrm{s}) - \left[\Delta H_{f}^{0}(\mathrm{Na}_{2}\mathrm{O}, \mathrm{s}) + \Delta H_{f}^{0}(\mathrm{H}_{2}\mathrm{O}, \mathrm{l})\right] = 2 \cdot (-427.8) - \\
& -[-416 + (-286)] = -153.6 \text{ kJ. }
\end{aligned}
$$

Present the answer in LaTex format: \boxed{Your answer}
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