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89. Consider this reaction occurring at 298 K: N2O(g) + NO2(g) 3 NO(g) a. Show that the reaction is not spontaneous under standard conditions by calculating A Grxn b. If a reaction mixture contains only N2O and NO2 at partial pressures of 1.0 atm each, the reaction will be spontane- ous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous? c. Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, what temperature is required to make the reaction spontaneous under standard conditions?

89. Consider this reaction occurring at 298 K: N2O(g) + NO2(g) 3 NO(g) a. Show that the reaction is not spontaneous under standard conditions by calculating A Grxn b. If a reaction mixture contains only N2O and NO2 at partial pressures of 1.0 atm each, the reaction will be spontane- ous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous? c. Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, what temperature is required to make the reaction spontaneous under standard conditions?

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
Problem 50PS
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89. Consider this reaction occurring at 298 K: N2O(g) + NO2(g) 3 NO(g) a. Show that the reaction is not spontaneous under standard conditions by calculating A Grxn b. If a reaction mixture contains only N2O and NO2 at partial pressures of 1.0 atm each, the reaction will be spontane- ous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous? c. Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, what temperature is required to make the reaction spontaneous under standard conditions?
Transcribed Image Text:89. Consider this reaction occurring at 298 K: N2O(g) + NO2(g) 3 NO(g) a. Show that the reaction is not spontaneous under standard conditions by calculating A Grxn b. If a reaction mixture contains only N2O and NO2 at partial pressures of 1.0 atm each, the reaction will be spontane- ous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous? c. Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, what temperature is required to make the reaction spontaneous under standard conditions?
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