Nitric acid is produced commercially by the Ostwald process,represented by the f

Question

Nitric acid is produced commercially by the Ostwald process,represented by the following equations: 4NH3(g) + 5O2(g) -----> 4NO(g) +6H2O 2NO(g) + O2(g) ------> 2NO2(g) 3NO2(g) + H2O(l) -------->2HNO3(aq) + NO(g) What mass of NH3 must be used to produce 1.0 x106 kg HNO3 by the Ostwald process? Assume100% yield in each reaction and assume the NO produced in the thirdstep is not recycled. Nitric acid is produced commercially by the Ostwald process,represented by the following equations: 4NH3(g) + 5O2(g) -----> 4NO(g) +6H2O 2NO(g) + O2(g) ------> 2NO2(g) 3NO2(g) + H2O(l) -------->2HNO3(aq) + NO(g) What mass of NH3 must be used to produce 1.0 x106 kg HNO3 by the Ostwald process? Assume100% yield in each reaction and assume the NO produced in the thirdstep is not recycled.

Explanation / Answer

4NH3(g) + 5O2(g) -----> 4NO(g) +6H2O                                        ----------------(1) 2NO(g) + O2(g) ------>2NO2(g)                                                      ----------------(2) 3NO2(g) + H2O(l) -------->2HNO3(aq) +NO(g)                           -----------------(3) The overall reaction is given by Eq(1) + 2* Eq(2)+ (4/3) Eq(3) we get 12NH3(g) + 21O2(g)   --------> 8HNO3(aq) +4 NO(g)   + 14H2O(l) Mol. wt. of NH3 is = 14 + 3 ( 1) = 17 g Mol. wt . of HNO3 is = 1 + 14 + 3 ( 16 ) = 63g 12 * 17 g of NH3 produces 8* 63 g ofHNO3 204 g of NH3 produces 504 g ofHNO3 0.204 Kg of NH3 produces 0.504 Kg of HNO3 X Kg of NH3 produces 1.0 x106 kg of HNO3 X = (1.0 x 106 kg * 0.204 Kg ) / 0.504Kg    = 0.4047 * 106 kg X = (1.0 x 106 kg * 0.204 Kg ) / 0.504Kg    = 0.4047 * 106 kg

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