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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: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter15: Complex Ion And Precipitation Equilibria
Section: Chapter Questions
Problem 60QAP: Consider the following hypothetical dissociation: AB3(s) A3+(aq)+3 B(aq)H0What effect will each of...
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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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