5 Ammonia is converted into nitrogen() oxide in industry by the Ostwald process: 4NH:(9) + 50:(9) = 4NO(g) + 6H;O(g) AH = -905.2 kJ mol The reaction is normally carried out at a pressure of around 500 kPa. a Use ideas about equilibrium to explain why pressures above 500 kPa are not used in industry for the Ostwald process. - -- b 200 moles of ammonia and 600 moles of oxygen are placed ina reactor at 600 K and a pressure of 500 kPa. At equilibrium, 100 moles of nitrogen(11) oxide have formed. Calculate a value for the equilibrium constant, K, including units, for this equilibrium. Give your answer to an appropriate number of significant figures.

5 Ammonia is converted into nitrogen() oxide in industry by the Ostwald process: 4NH:(9) + 50:(9) = 4NO(g) + 6H;O(g) AH = -905.2 kJ mol The reaction is normally carried out at a pressure of around 500 kPa. a Use ideas about equilibrium to explain why pressures above 500 kPa are not used in industry for the Ostwald process. - -- b 200 moles of ammonia and 600 moles of oxygen are placed ina reactor at 600 K and a pressure of 500 kPa. At equilibrium, 100 moles of nitrogen(11) oxide have formed. Calculate a value for the equilibrium constant, K, including units, for this equilibrium. Give your answer to an appropriate number of significant figures.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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