Nitric acid is produced commercially by the Ostwald process. In the first step ammonia is oxidized to nitric oxide: 4NH3(g) +502 (9)→ 4NO(g) + 6H₂O(g) Assume this reaction is carried out in the apparatus diagramed below. 3.00 L NH3 0.500 atm 100 1.50 L 0₂ 1.50 atm The stopcock between the two reaction containers is opened, and the reaction proceeds using proper catalysts. Calculate the partial pressure of NO after the reaction is complete. Assume 100% yield for the reaction, assume the final container volume is 4.50 L, and assume the temperature is constant. Partial pressure of NO = atm
Nitric acid is produced commercially by the Ostwald process. In the first step ammonia is oxidized to nitric oxide: 4NH3(g) +502 (9)→ 4NO(g) + 6H₂O(g) Assume this reaction is carried out in the apparatus diagramed below. 3.00 L NH3 0.500 atm 100 1.50 L 0₂ 1.50 atm The stopcock between the two reaction containers is opened, and the reaction proceeds using proper catalysts. Calculate the partial pressure of NO after the reaction is complete. Assume 100% yield for the reaction, assume the final container volume is 4.50 L, and assume the temperature is constant. Partial pressure of NO = atm
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter19: The Representative Elements
Section: Chapter Questions
Problem 104CP
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Transcribed Image Text:Nitric acid is produced commercially by the Ostwald process. In the first step ammonia is oxidized to nitric oxide:
4NH3(g) +502 (9) → 4NO(g) + 6H₂O(g)
Assume this reaction is carried out in the apparatus diagramed below.
0+0
3.00 L NH3
0.500 atm
1.50 L 0₂
1.50 atm
The stopcock between the two reaction containers is opened, and the reaction proceeds using proper catalysts. Calculate the partial pressure of NO after the reaction is complete. Assume
100% yield for the reaction, assume the final container volume is 4.50 L, and assume the temperature is constant.
Partial pressure of NO =
atm
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