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The following sequence of reactions occurs in the commercial production of aqueous nitric acid. (The overall industrial process produces excess NO.) 4 NH3(g) + 5 02(g) -> 4 NO(g) + 6 H20(/) AH = -1166.0 kJ/mol (1) 2 NO(g) + 02(g) -> 2 NO2(g)AH = -116.2 kJ/mol (2) 3 NO2(g) + H20(/) -> 2 HNO3(aq) + NO(g) OH = -137.3 kJ/mol (3) Determine the total energy change (in kJ) for the production of one mole of aqueous nitric acid by this proces