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2.0 x 10-31 at 25 °C a. Calculate the partial pressure of NO at equilibrium if the initial partial pressures of N₂ and O₂ are 0.78 atm and 0.21 atm, respectively. (10)

2.0 x 10-31 at 25 °C a. Calculate the partial pressure of NO at equilibrium if the initial partial pressures of N₂ and O₂ are 0.78 atm and 0.21 atm, respectively. (10)

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
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 34QAP: At 500C, k for the for the formation of ammonia from nitrogen and hydrogen gases is 1.5105....
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Solve correctly please. (Gpt/ai wrong answer not allowed)
3. In the atmosphere, nitrogen reacts with oxygen to form NO, perhaps best known as "laughing gas". The reaction and its equilibrium constant (K) is K₂= 2.0 x 10-31 at 25 °C a. Calculate the partial pressure of NO at equilibrium if the initial partial pressures of N₂ and O₂ are 0.78 atm and 0.21 atm, respectively. (10) N₂(g) + O₂(g) 2NO(g) b. What is the value of K. at this temperature?
Transcribed Image Text:3. In the atmosphere, nitrogen reacts with oxygen to form NO, perhaps best known as "laughing gas". The reaction and its equilibrium constant (K) is K₂= 2.0 x 10-31 at 25 °C a. Calculate the partial pressure of NO at equilibrium if the initial partial pressures of N₂ and O₂ are 0.78 atm and 0.21 atm, respectively. (10) N₂(g) + O₂(g) 2NO(g) b. What is the value of K. at this temperature?
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