5.3 Exercise 21

The following sequence of reactions occurs in the commercial production of aqueous nitric acid:
$4 \text{NH}_{3} \left(g\right) + 5 \text{O}_{2} \left(g\right) \rightarrow 4 \text{NO} \left(g\right) + 6 \text{H}_{2} \text{O} \left(l\right) \Delta \text{H} = −907 \text{kJ}$
$2 \text{NO} \left(g\right) + \text{O}_{2} \left(g\right) \rightarrow 2 \text{NO}_{2} \left(g\right) \Delta \text{H} = −113 \text{kJ}$
$3 \text{NO}_{2} + \text{H}_{2} \text{O} \left(l\right) \rightarrow 2 \text{HNO}_{3} \left(a q\right) + \text{NO} \left(g\right) \Delta \text{H} = −139 \text{kJ}$

Determine the total enthalpy change for the production of one mole of aqueous nitric acid by this process. Coproducts of the net reaction include water and nitrogen monoxide.