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12. In the Ostwald process for oxidizing ammonia, a variety of products is possible - N₂, N₂O, NO, and NO₂- depending on the conditions. One possibility is: NH3(g) + O₂(g) = NO(g) + H₂O (g) Kp = 2.11 x 10¹⁹ at 700 K For the decomposition of NO2 at 700 K, NO2(g) = NO(g) + O2(g) Kp = 0.524 at 700 K What is K, for the oxidation of NH3(g) to NO2(g)? 13. The decomposition of N₂O4 to NO₂ is represented by the equilibrium reaction equation below N2O4(g) 2 NO2 (g) If 1.75 moles of N₂O4 is injected in a 1.5 L vessel and at equilibrium 25% N₂O4 is dissociated, what is the equilibrium constant for this reaction?

12. In the Ostwald process for oxidizing ammonia, a variety of products is possible - N₂, N₂O, NO, and NO₂- depending on the conditions. One possibility is: NH3(g) + O₂(g) = NO(g) + H₂O (g) Kp = 2.11 x 10¹⁹ at 700 K For the decomposition of NO2 at 700 K, NO2(g) = NO(g) + O2(g) Kp = 0.524 at 700 K What is K, for the oxidation of NH3(g) to NO2(g)? 13. The decomposition of N₂O4 to NO₂ is represented by the equilibrium reaction equation below N2O4(g) 2 NO2 (g) If 1.75 moles of N₂O4 is injected in a 1.5 L vessel and at equilibrium 25% N₂O4 is dissociated, what is the equilibrium constant for this reaction?

Chemistry & Chemical Reactivity
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
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 38GQ: At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g)...
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12. In the Ostwald process for oxidizing ammonia, a variety of products is possible - N2, N₂O, NO, and NO₂- depending on the conditions. One possibility is: NH3(g) + O₂(g) = NO(g) + H₂O (g) Kp = 2.11 x 10¹⁹ at 700 K For the decomposition of NO2 at 700 K, NO₂(g) = NO(g) + O2(g) Kp = 0.524 at 700 K What is Kp for the oxidation of NH3(g) to NO2(g)? 13. The decomposition of N₂O4 to NO₂ is represented by the equilibrium reaction equation below N2O4(g) 2 NO2 (g) If 1.75 moles of N₂O4 is injected in a 1.5 L vessel and at equilibrium 25% N₂O4 is dissociated, what is the equilibrium constant for this reaction?
Transcribed Image Text:12. In the Ostwald process for oxidizing ammonia, a variety of products is possible - N2, N₂O, NO, and NO₂- depending on the conditions. One possibility is: NH3(g) + O₂(g) = NO(g) + H₂O (g) Kp = 2.11 x 10¹⁹ at 700 K For the decomposition of NO2 at 700 K, NO₂(g) = NO(g) + O2(g) Kp = 0.524 at 700 K What is Kp for the oxidation of NH3(g) to NO2(g)? 13. The decomposition of N₂O4 to NO₂ is represented by the equilibrium reaction equation below N2O4(g) 2 NO2 (g) If 1.75 moles of N₂O4 is injected in a 1.5 L vessel and at equilibrium 25% N₂O4 is dissociated, what is the equilibrium constant for this reaction?
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