A student investigating the thermodynamics of nitrogen oxides compiles the thermochemical data shown in the table below. | Reaction | \(\Delta H^\circ\ (\text{kJ/mol}_{\text{rxn}})\) | |---|---| | \(2\text{NO}(g) + \text{O}_2(g) \rightarrow 2\text{NO}_2(g)\) | \(-114\) | | \(2\text{N}_2\text{O}(g) \rightarrow 2\text{N}_2(g) + \text{O}_2(g)\) | \(-164\) | | \(\text{N}_2(g) + \text{O}_2(g) \rightarrow 2\text{NO}(g)\) | \(+180\) | Based on the data, what is the value of \(\Delta H^\circ\) for the reaction \(\text{N}_2\text{O}(g) + \text{NO}_2(g) \rightarrow 3\text{NO}(g)\) ? • Nerd Notes

AP Chemistry

6.9 Hess’s Law

IntermediateMCQMathematical22.7k

A student investigating the thermodynamics of nitrogen oxides compiles the thermochemical data shown in the table below.

Reaction	\(\Delta H^\circ\ (\text{kJ/mol}_{\text{rxn}})\)
\(2\text{NO}(g) + \text{O}_2(g) \rightarrow 2\text{NO}_2(g)\)	\(-114\)
\(2\text{N}_2\text{O}(g) \rightarrow 2\text{N}_2(g) + \text{O}_2(g)\)	\(-164\)
\(\text{N}_2(g) + \text{O}_2(g) \rightarrow 2\text{NO}(g)\)	\(+180\)

Based on the data, what is the value of \(\Delta H^\circ\) for the reaction \(\text{N}_2\text{O}(g) + \text{NO}_2(g) \rightarrow 3\text{NO}(g)\) ?

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