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mperature with oxygen in a reversible, exothermic reaction: 4 NH3(g) + 5 0₂(g) 4 NO(g) + 6 H₂O(g) State and explain the effect of an increase in pressure on the equilibrium position. State and explain the effect of an increase in temperature on this equilibrium position. i) ii)

mperature with oxygen in a reversible, exothermic reaction: 4 NH3(g) + 5 0₂(g) 4 NO(g) + 6 H₂O(g) State and explain the effect of an increase in pressure on the equilibrium position. State and explain the effect of an increase in temperature on this equilibrium position. i) ii)

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter13: Fundamental Equilibrium Concepts
Section: Chapter Questions
Problem 12E: Show that the complete chemical equation, the total ionic equation, and the net ionic equation for...
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Question 2 a) In the first stage of the industrial production of nitric acid, ammonia reacts at high temperature with oxygen in a reversible, exothermic reaction: 4 NH3(g) + 5 O₂(g) 4 NO(g) + 6 H₂O(g) State and explain the effect of an increase in pressure on the equilibrium position. State and explain the effect of an increase in temperature on this equilibrium position. i) ii)
Transcribed Image Text:Question 2 a) In the first stage of the industrial production of nitric acid, ammonia reacts at high temperature with oxygen in a reversible, exothermic reaction: 4 NH3(g) + 5 O₂(g) 4 NO(g) + 6 H₂O(g) State and explain the effect of an increase in pressure on the equilibrium position. State and explain the effect of an increase in temperature on this equilibrium position. i) ii)
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