Nitric acid is manufactured in the Oswald process, which involves the catalytic oxidation of ammonia according to the following equations: (i) 4 NH3(g) + 5 02(g) → 4 NO(g) + 6 H2O(g) (ii) 2 NO(g) + O2(g) → 2 NO2(g); (iii) 3 NO2(g) + H2O(1) → 2 HNO;(aq) + NO(g); (NO is fed back into the second reactor) (a) The above equations may be combined to yield the following equation. Balance this equation. _NH3(g) + _O2(g) + _H2O(!) _HNO3() + _H2O(1) + __NO(g) (b) What is the mole fraction of NH3 that becomes nitric acid in one reaction cycle? (c) How many kilograms of HNO; will be produced in one reaction cycle from 1.00 m³ of NH3, measured at STP, if the overall yield is 92.0%? (d) If concentrated nitric acid contains 70.0% (by mass) of HNO; and the solution has density of 1.48 g/mL, how many litters of concentrated nitric acid is produced in this process at the above reaction yield? (Answers: (b) 2/3; (c) 1.73 kg of HNO3; (d) 1.67 L)
Nitric acid is manufactured in the Oswald process, which involves the catalytic oxidation of ammonia according to the following equations: (i) 4 NH3(g) + 5 02(g) → 4 NO(g) + 6 H2O(g) (ii) 2 NO(g) + O2(g) → 2 NO2(g); (iii) 3 NO2(g) + H2O(1) → 2 HNO;(aq) + NO(g); (NO is fed back into the second reactor) (a) The above equations may be combined to yield the following equation. Balance this equation. _NH3(g) + _O2(g) + _H2O(!) _HNO3() + _H2O(1) + __NO(g) (b) What is the mole fraction of NH3 that becomes nitric acid in one reaction cycle? (c) How many kilograms of HNO; will be produced in one reaction cycle from 1.00 m³ of NH3, measured at STP, if the overall yield is 92.0%? (d) If concentrated nitric acid contains 70.0% (by mass) of HNO; and the solution has density of 1.48 g/mL, how many litters of concentrated nitric acid is produced in this process at the above reaction yield? (Answers: (b) 2/3; (c) 1.73 kg of HNO3; (d) 1.67 L)
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 129AE: One of the few industrial-scale processes that produce organic compounds electrochemically is used...
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Transcribed Image Text:21. Nitric acid is manufactured in the Oswald process, which involves the catalytic oxidation of ammonia
according to the following equations:
(i) 4 NH3(g) + 5 O2(g)
→ 4 NO(g) + 6 H2O(g)
(ii) 2 NO(g) + O2(8)
2 NO2(g);
(iii) 3 NO2(g) + H2O(1)
→ 2 HNO3(aq) + NO(g); (NO is fed back into the second reactor)
(a) The above equations may be combined to yield the following equation. Balance this equation.
NH3(g) +_O2(g) +
_H2O(1)
_HNO3(1) + _H,O(1) +
NO(g)
(b) What is the mole fraction of NH3 that becomes nitric acid in one reaction cycle?
(c) How many kilograms of HNO3 will be produced in one reaction cycle from 1.00 m³ of NH3,
measured at STP, if the overall yield is 92.0%?
(d) If concentrated nitric acid contains 70.0% (by mass) of HNO3 and the solution has density of 1.48
g/mL, how many litters of concentrated nitric acid is produced in this process at the above reaction
yield? (Answers: (b) 2/3; (c) 1.73 kg of HNO3; (d) 1.67 L)
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