Certainly! To complete the thermochemical reactions with the correct enthalpy changes, we'll place the provided enthalpy changes in the appropriate locations within the given chemical equations.
1. For the reaction:
[tex]\[
N_2(g) + O_2(g) \rightarrow 2 H_2(\theta) \quad \text{+} \quad 180.58 \, \text{kJ}
\][/tex]
2. For the reaction:
[tex]\[
2 H_2(\theta) + O_2(\theta) \rightarrow 2 H_2O(\theta) \quad \text{+} \quad 570.6 \, \text{kJ}
\][/tex]
So, the completed thermochemical reactions with the correct enthalpy changes are:
[tex]\[
\begin{aligned}
1.\quad &N_2(g) + O_2(g) \rightarrow 2 H_2(\theta) &\quad \text{+} \quad 180.58 \, \text{kJ} \\
2.\quad &2 H_2(\theta) + O_2(\theta) \rightarrow 2 H_2O(\theta) &\quad \text{+} \quad 570.6 \, \text{kJ}
\end{aligned}
\][/tex]
These enthalpy values represent the heat absorbed or released during each reaction.
