Applying Hess's Law
Consider the chemical equations shown here:
$\begin{array}{l}
NO(g)+O_3(g) \rightarrow NO_2(g)+O_2(g) \quad \Delta H_1=-198.9\text{ kJ} \\
\frac{3}{2} O_2(g) \rightarrow O_3(g) \quad \Delta H_2=142.3\text{ kJ} \\
O(g) \rightarrow \frac{1}{2} O_2(g) \quad \Delta H_3=-247.5\text{ kJ}
\end{array}$
What is $\Delta H_{\text{rxn}}$ for the reaction shown?
$NO(g)+O(g) \rightarrow NO_2(g)$
Consider the chemical equations shown here:
$\begin{array}{l}
NO(g)+O_3(g) \rightarrow NO_2(g)+O_2(g) \quad \Delta H_1=-198.9\text{ kJ} \\
\frac{3}{2} O_2(g) \rightarrow O_3(g) \quad \Delta H_2=142.3\text{ kJ} \\
O(g) \rightarrow \frac{1}{2} O_2(g) \quad \Delta H_3=-247.5\text{ kJ}
\end{array}$
What is $\Delta H_{\text{rxn}}$ for the reaction shown?
$NO(g)+O(g) \rightarrow NO_2(g)$