Industrially, nitric acid is produced by the Ostwald process, as represented by the following equations: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(l) 2NO(g) + O2(g) → 2NO2(g) 2NO2(g) + H2O(l) → HNO3(aq) + HNO2(aq) What mass of NH3 (in grams) must be used to produce 4.65 tons of HNO3 by the Ostwald process, assuming an 80.0 percent yield in each step (1 ton = 2000 lb; 1 lb = 453.6 g)? Enter your answer in scientific notation.
Industrially, nitric acid is produced by the Ostwald process, as represented by the following equations: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(l) 2NO(g) + O2(g) → 2NO2(g) 2NO2(g) + H2O(l) → HNO3(aq) + HNO2(aq) What mass of NH3 (in grams) must be used to produce 4.65 tons of HNO3 by the Ostwald process, assuming an 80.0 percent yield in each step (1 ton = 2000 lb; 1 lb = 453.6 g)? Enter your answer in scientific notation.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter21: The Chemistry Of The Main Group Elements
Section: Chapter Questions
Problem 76GQ
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Industrially, nitric acid is produced by the Ostwald process, as represented by the following equations:
What mass of NH3 (in grams) must be used to produce 4.65 tons of HNO3 by the Ostwald process, assuming an 80.0 percent yield in each step (1 ton = 2000 lb; 1 lb = 453.6 g)? Enter your answer in scientific notation. |
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