Question

The following sequence of reactions occurs in the commercial production of aqueous nitric acid:4NH3(g) + 5O2(g) ⟶ 4NO(g) + 6H2 O(l) ΔH = −907 kJ
2NO(g) + O2(g) ⟶ 2NO2(g) ΔH = −113 kJ
3NO2 + H2 O(l) ⟶ 2HNO3(aq) + NO(g) ΔH = −139 kJ

Determine the total energy change for the production of one mole of aqueous nitric acid by this process.

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