The following sequence of reaction occurs in commercial production of aqueous nitric acid. 4NH3(g)+5O2(g)→4NO(g)+6H2O(l) ΔH=−904 kJ ...(1) 2NO(g)+O2(g)→2NO2(g) ΔH=−112 kJ ...(2) 3NO2(g)+H2O(l)→2HNO3(aq)+NO(g) ΔH=−140 kJ ...(3) Determine the magnitude of total heat (in kJ/mole) liberated at constant pressure for the production of exactly 1 mole of aqueous nitric acid by this process

The following sequence of reaction occurs in commercial production of

1.	The following sequence of reaction occurs in commercial production of aqueous nitric acid. 4NH3(g)+5O2(g)→4NO(g)+6H2O(l) ΔH=−904 kJ ...(1) 2NO(g)+O2(g)→2NO2(g) ΔH=−112 kJ ...(2) 3NO2(g)+H2O(l)→2HNO3(aq)+NO(g) ΔH=−140 kJ ...(3) Determine the magnitude of total heat (in kJ/mole) liberated at constant pressure for the production of exactly 1 mole of aqueous nitric acid by this process
Answer» The following sequence of reaction occurs in commercial production of aqueous nitric acid. $4 N H_{3} (g) + 5 O_{2} (g) \to 4 N O (g) + 6 H_{2} O (l) Δ H = - 904 k J . . . (1)$ $2 N O (g) + O_{2} (g) \to 2 N O_{2} (g) Δ H = - 112 k J . . . (2)$ $3 N O_{2} (g) + H_{2} O (l) \to 2 H N O_{3} (a q) + N O (g) Δ H = - 140 k J . . . (3)$ Determine the magnitude of total heat $(i n kJ/mole)$ liberated at constant pressure for the production of exactly 1 mole of aqueous nitric acid by this process